Answer:
B
Explanation:
The rate law is a way for us to measure the rate of a given reaction by comparing it to the concentration of the reactants. Based on the mole ratios of the reactants, we can hypothesize that adding more reactant will speed up the rate of reaction due to the simple principle that if there is more of an opportunity for molecules or atoms to collide, then the rate of reaction will be faster. Hope that helps :)
A rate law is an equation that relates the reaction rate to the concentrations of the component reactants.
Rate lawsIn chemistry, rate laws are mathematical expressions that relate the rate of a reaction to the concentrations of the component reactants in the reaction.
For example, consider the following reaction:
A + B -----------> C + D
The rate law for the reaction is given as:
Rate = k[tex][A]^m[B]^n[/tex] where k = rate constant and m/n = order of reactions.
More on rate laws can be found here: https://brainly.com/question/4222261
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Given that the molar mass of NAOH is 40.00G/MOL, what mass of NAOH is needed to make 2.500 L of a 2.000 M NaOH Solution?
Answer:
200g
Explanation:
n = CV
n = mass/molar mass
mass/molar mass = CV
mass/40 = 2 x 2.5
mass/40 = 5
mass = 5x 40
mass = 200g
Name the following alkanes. Please need help last assignment. The questions in the picture.
Answer:
Hydrogen, carbon reaction
Covalent bonding occurs between two oxygen atoms to form O2. What's the partial charge on each oxygen atom in 02?
A. Both oxygen atoms have positive partial charge.
B. Both oxygen atoms have negative partial charge.
C. Both oxygen atoms have zero partial charge.
D. One oxygen atom has positive partial charge, and the other has negative partial charge.
Answer:
Both oxygen atoms have zero partial charge.
Explanation:
In covalent bonds, electrons are shared between the two bonding atoms. The shared electron pair of the covalent bond is positioned between the nuclei of the two bonding atoms.
A covalent bond may be formed between two or more elements of different electronegativities. When a difference in electro negativity exists between these atoms in a covalent bond, the molecule becomes polarized. The shared electron pair of the covalent bond becomes closer to the nucleus of the more electronegative atom (s). This more electronegative atom (s) becomes partially negative while the other atom becomes partially positive.
When the two bonding atoms are of equal electronegativities such that the electro negativity difference between the bonding atoms is zero, there is now no difference in electro negativity and no consequent partial charges.
Since the two oxygen atoms have the same electro negativity, there is no difference in electronegativity, hence there is no partial charge between the two oxygen atoms.
Answer:
Both oxygen atoms have zero partial charge.
Explanation:
Identify the particle that must receive 2 electrons to acquire a charge of +1. a) K b) Fe2+ c) O2- d) Nee) Al3+ (URGENT) Needs to be done in 30 mins
Answer:
E) Al³⁺
Explanation:
A reaction involving a gain of electrons is known as a reduction reaction because the oxidation number of the species gaining the electron is reduced.
In the given question, the oxidation number (charge) of particle accepting two electrons will decrease by 2. From the given options;
A. K is a neutral atom with oxidation number of 0. If is accepts two electrons, its oxidation number becomes -2.
K + 2e⁻ ----> K⁻²
B) Fe²⁺ has a charge of +2. If it accepts two electrons, its charge comes 0.
Fe⁺ + 2e⁻ ----> Fe
C) O²⁻ has a charge of -2. if it accepts two electrons, it will have a charge of -4.
O²⁻ + 2e⁻ ----> O⁴⁻
D) Ne has a charge of zero. If it accepts two electrons, its charge becomes -2.
Ne + 2e⁻ ----> Ne²⁻
E) Al³⁺ has a charge of +3. If it gains two electrons, its charge becomes +1.
Al³⁺ + 2e⁻ ----> Al⁺
Using bond energies, estimate the enthalpy of reaction for the following chemical reaction. CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g) ΔHrxn = ?
Answer:
[tex]\mathbf{ \Delta H_{rxn} = -1936 \ kJ/mol}}[/tex]
Explanation:
The equation for the reaction is given as:
[tex]\mathbf{ CH_{4(g)} + 4 F_{2(g)} \to CF_{4(g)} + 4 HF_{(g) }}[/tex]
At standard conditions; the bond energies are as follows;
Bond Bond Energies (kJ/mol)
C-H 413
F-F 155
C-F 485
H-F 567
[tex]\mathbf{\Delta \ H_{rxn} = \sum \Delta H ( reactant) - \sum \Delta H (product)}[/tex]
[tex]\mathbf{\Delta \ H_{rxn} = \sum [\Delta H \ 4( C-H) + \Delta H \ 4(F-F) ]- \sum[ \Delta H \ 4( C-F)+\Delta H \ 4( H-F)] (product)}[/tex]
[tex]\mathbf{\Delta \ H_{rxn} = \sum{ \Delta \ H (4*413) + \Delta \ H (4*155) - \Delta \ H (4(485)) + \Delta H (4(567) }}[/tex]
[tex]\mathbf{ \Delta H_{rxn} = \sum ({ (1652 + 620) - (1940 + 2268)})}[/tex]
[tex]\mathbf{ \Delta H_{rxn} = \sum ({2272- 4208})}[/tex]
[tex]\mathbf{ \Delta H_{rxn} = -1936 \ kJ/mol}}[/tex]
An ion of a single pure element always has an oxidation number of ________.
Answer: An ion of a single pure element always has an oxidation number of
zero.
Explanation:
Use the reaction I2(s) I2(g), H = 62.4 kJ/mol, S = 0.145 kJ/(molK)
At what temperature is the reaction at equilibrium?
A.157K
B.430K
C.0.002K
D.62K
Answer: B. 430 K
Explanation:
According to Gibb's equation:
[tex]\Delta G=\Delta H-T\Delta S[/tex]
[tex]\Delta G[/tex] = Gibbs free energy
[tex]\Delta H[/tex] = enthalpy change = +62.4 kJ/mol
[tex]\Delta S[/tex] = entropy change = +0.145 kJ/molK
T = temperature in Kelvin
[tex]\Delta G[/tex] = +ve, reaction is non spontaneous
[tex]\Delta G[/tex] = -ve, reaction is spontaneous
[tex]\Delta G[/tex] = 0, reaction is in equilibrium
[tex]\Delta H-T\Delta S=0[/tex] for reaction to be spontaneous
[tex]T=\frac{\Delta H}{\Delta S}[/tex]
[tex]T=\frac{62.4kJ/mol}{0.145kJ/molK}=430K[/tex]
Thus the Reaction is spontaneous when temperature is 430 K.
Answer:
430 K
Explanation:
i just took the test on a pex :)
Observing Gas Properties - Flammability
Chemicals Observations
HCl
Zn
HCl + Zn Reaction
Gas + Flame
Conclusion:
A. When performing this experiment, when is the tetradecanol in a condensed phase? Explain your answer.
B. The published melting point of H2O is 0°C, and the published boiling point is 100°C. Why would you have found slightly different values?
C. In this experiment, there were two possible identities for the gas produced: hydrogen or chlorine, which have quite different properties. Hydrogen is a colorless, odorless, flammable gas. Chlorine gas is greenish yellow with a pungent, bleach-like odor and is non-flammable. Use your observations to determine which gas was produced in this experiment.
D. Give some examples of how it might be useful to know the melting or boiling points of a substance. Think in terms of both scientific and commercial/industrial settings.
Answer:
The answer is C love.
Explanation:
Answer:
a) It is when a solid is going into the liquid stage. The molecules are really close together.
b) The water could have impurities, altitude could effect the boiling point or the temperature could of been measured wrong.
c) The gas was colorless and odorless therefore it is Hydrogen gas.
d) In a Scientific setting finding the boiling point of a new unknown substances can help identify and organize them. In a commercial setting chemicals need to be stored a certain way according to their boiling point. Stored incorrectly could cause the substance to evaporate.
Brown algae, such as giant kelp and sargassum, are an example of ? A. macroalgae B chemosynthetic algae C Flowering plants D Phytoplankton
Answer:
The answer is option A.
I hope this helps you.
Answer:
Macro Algae
Explanation:
probz
Which of the following does pascal's Principle help to explain?
Answer:
B) hydraulics
Explanation:
Answer:
hydraulics
Explanation:
i got it right the test on apex
:DDDDDDDD
After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? The value of Kf for Ni(NH3)62+ is 2.0×108. Express the concentration to two significant figures and include the appropriate units.
Answer:
[tex]\large \boxed{1.77 \times 10^{-5}\text{ mol/L}}[/tex]
Explanation:
Assume that you have mixed 135 mL of 0.0147 mol·L⁻¹ NiCl₂ with 190 mL of 0.250 mol·L⁻¹ NH₃.
1. Moles of Ni²⁺
[tex]n = \text{135 mL} \times \dfrac{\text{0.0147 mmol}}{\text{1 mL}} = \text{1.984 mmol}[/tex]
2. Moles of NH₃
[tex]n = \text{190 mL} \times \dfrac{\text{0.250 mmol}}{\text{1 mL}} = \text{47.50 mmol}[/tex]
3. Initial concentrations after mixing
(a) Total volume
V = 135 mL + 190 mL = 325 mL
(b) [Ni²⁺]
[tex]c = \dfrac{\text{1.984 mmol}}{\text{325 mL}} = 6.106 \times 10^{-3}\text{ mol/L}[/tex]
(c) [NH₃]
[tex]c = \dfrac{\text{47.50 mmol}}{\text{325 mL}} = \text{0.1462 mol/L}[/tex]
3. Equilibrium concentration of Ni²⁺
The reaction will reach the same equilibrium whether it approaches from the right or left.
Assume the reaction goes to completion.
Ni²⁺ + 6NH₃ ⇌ Ni(NH₃)₆²⁺
I/mol·L⁻¹: 6.106×10⁻³ 0.1462 0
C/mol·L⁻¹: -6.106×10⁻³ 0.1462-6×6.106×10⁻³ 0
E/mol·L⁻¹: 0 0.1095 6.106×10⁻³
Then we approach equilibrium from the right.
Ni²⁺ + 6NH₃ ⇌ Ni(NH₃)₆²⁺
I/mol·L⁻¹: 0 0.1095 6.106×10⁻³
C/mol·L⁻¹: +x +6x -x
E/mol·L⁻¹: x 0.1095+6x 6.106×10⁻³-x
[tex]K_{\text{f}} = \dfrac{\text{[Ni(NH$_{3}$)$_{6}^{2+}$]}}{\text{[Ni$^{2+}$]}\text{[NH$_{3}$]}^{6}} = 2.0 \times 10^{8}[/tex]
Kf is large, so x ≪ 6.106×10⁻³. Then
[tex]K_{\text{f}} = \dfrac{\text{[Ni(NH$_{3}$)$_{6}^{2+}$]}}{\text{[Ni$^{2+}$]}\text{[NH$_{3}$]}^{6}} = 2.0 \times 10^{8}\\\\\dfrac{6.106 \times 10^{-3}}{x\times 0.1095^{6}} = 2.0 \times 10^{8}\\\\6.106 \times 10^{-3} = 2.0 \times 10^{8}\times 0.1095^{6}x= 345.1x\\x= \dfrac{6.106 \times 10^{-3}}{345.1} = 1.77 \times 10^{-5}\\\\\text{The concentration of Ni$^{2+}$ at equilibrium is $\large \boxed{\mathbf{1.77 \times 10^{-5}}\textbf{ mol/L}}$}[/tex]
The force that opposes drag and is powered by combustion reactions in the
engine is
Answer:
Thrust.
Explanation:
hope this helps you :)
Answer:
thrust
Explanation:
4. In which pair of substances does the first underlined atom have a lower oxidation number than the second? A. NH3OH+ NH4– B. H2O H2O2 C. SO3 SO42– D. HCHO C
Answer:
Option B is correct.
Only this option has the first underlined element with a lower oxidation number than the second amongst the options.
Explanation:
Complete Question
In which pair of substances does the first underlined atom have a lower oxidation number than the second?
A. NH₃OH⁺, NH₄⁻ (N is underlined)
B. H₂O, H₂O₂ (O is underlined)
C. SO₃, SO₄²⁻ (S is underlined)
D. HCHO, C (C is underlined)
Solution
In determination of the oxidation number of an atom in a compound, we first name the unknown oxidation number x.
Then, the total oxidation number of the atoms in the compound is equal to the charge of on the compound (or radical).
So, elements in their neutral state have no charge and no oxidation number.
A. NH₃OH⁺, NH₄⁻ (N is underlined)
N in NH₃OH⁺
Oxidation number of N = x
Oxidation number of H = +1
Oxidation number of O = -2
x + (3×+1) + (-2) + (+1) = +1
x - 3 - 2 + 1 = 1
x = +5
N in NH₄⁻
Oxidation number of N = x
Oxidation number of H = +1
x + (4×1) = -1
x + 4 = -1
x = -1 - 4 = -5
First underlined element has a greater oxidation number than the second. So, this doesn't qualify.
B. H₂O, H₂O₂ (O is underlined)
O in H₂O
Oxidation number of H = +1
Oxidation number of O = x
(2×1) + x = 0
2 + x = 0
x = -2
H₂O₂
Oxidation number of H = +1
Oxidation number of O = x
(2×1) + (2×x) = 0
2 + 2x = 0
2x = -2
x = (-2/2) = -1.
First underlined element has a lower oxidation number than the second. So, this qualifies.
C. SO₃, SO₄²⁻ (S is underlined)
S in SO₃
Oxidation number of S = x
Oxidation number of O = -2
x + (3×-2) = 0
x - 6 = 0
x = +6
SO₄²⁻
Oxidation number of S = x
Oxidation number of O = -2
x + (4×-2) = -2
x - 8 = -2
x = 8 - 2 = +6
First underlined element has the same oxidation number as the second. So, this doesn't qualify.
D. HCHO, C (C is underlined)
C in HCHO
Oxidation number of H = +1
Oxidation number of C = x
Oxidation number of O = -2
+1 + x + 1 - 2 = 0
x = 0
C in C
Oxidation number of C = x
x = 0
First underlined element has the same oxidation number as the second. So, this doesn't qualify.
Hope this Helps!!!
What is the concentration (M) of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in sufficient water to give exactly 100. mL of solution
Answer:
[tex]3.65~M[/tex]
Explanation:
We have to remember the molarity equation:
[tex]M=\frac{mol}{L}[/tex]
So, we have to calculate "mol" and "L". The total volume is 100 mL. So, we can do the conversion:
[tex]100~mL\frac{1~L}{1000~mL}=~0.1~L[/tex]
Now we can calculate the moles. For this we have to calculate the molar mass:
O: 16 g/mol
H: 1 g/mol
C: 12 g/mol
[tex](16*1)+(1*4)+(12*1)=32~g/mol[/tex]
With the molar mass value we can calculate the number of moles:
[tex]1.7~g~of~CH_3OH\frac{1~mol~CH_3OH}{32~g~of~CH_3OH}=0.365~mol~CH_3OH[/tex]
Finally, we can calculate the molarity:
[tex]M=\frac{0.365~mol~CH_3OH}{0.1~L}=3.65~M[/tex]
I hope it helps!
Draw structural formulas for the major organic product(s) of the reaction shown below.
• You do not have to consider stereochemistry.
If no reaction occurs, draw the organic starting material.
Remember to include all of the formal charges on the atoms of any nitro groups.
Answer:
3-bromobenzoic acid
Explanation:
In this case, we have to remember that the [tex]Br_2/FeBr_3[/tex] is a reaction in which we add Br into the molecule an electrophilic aromatic substitution. Additionally, we have a carboxylic acid in the benzene. This carboxylic acid is an ortho director because is a deactivating group (it removes electrons from the benzene ring). With this in mind, a "Br" atom would be added in an ortho position respect to the COOH group and we will obtain 3-bromobenzoic acid.
See figure 1.
I hope it helps!
To create 3-bromobenzoic acid, a "Br" atom would be placed at an orthogonal position to the COOH group according to electrophilic aromatic substitution.
Electrophilic aromatic substitution is a type of organic reaction in which an atom or group in an aromatic ring is substituted with an electrophile. It is a fundamental reaction in aromatic chemistry that happens due to the aromatic system's high electron density.
It is an electrophilic aromatic substitution process in which Br is incorporated into the molecule. In addition, the benzene contains a carboxylic acid. Because it removes electrons from the benzene ring, this carboxylic acid functions as an ortho director. To create 3-bromobenzoic acid, a "Br" atom would be placed at an orthogonal position to the COOH group. The product is seen in the photographs below.
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If 50 ml of 1.00 M of H2SO4 and 50 ml of 2.0 M KOH are mixed what is the concentration of the resulting solutes?
Answer: [H2SO4] = 0.5M;
[KOH] = 1M
Explanation: Molarity is the solution concentration defined by:
molarity = [tex]\frac{mol}{L}[/tex] or M
To determine the concentration of the mixture, find how many mols of each compound there are in the mixture:
50 mL = 0.05L
H2SO4
1 mol/L * 0.05L = 0.05mol
KOH
2mol/L * 0.05L = 0.1 mol
The mixture has a total volume of:
V = 50 + 50 = 100 mL = 0.1 L
The concentration of the resullting solutes:
[H2SO4] = [tex]\frac{0.05}{0.1}[/tex] = 0.5 M
[KOH] = [tex]\frac{0.1}{0.1}[/tex] = 1 M
Concentration of H2SO4 is 0.5M while for KOH is 1M.
Which of the following would be useful for converting g/mol to g/L?
A. Mass percent
B. Avogadro's number
C. Molarity
D. Molar mass
Answer:
Molarity
Explanation:
The conversion of g/mol to g/L molarity can be used. Thus, option C is correct.
The g/mol has been the amount of solute present in a mole. The g/mol has been the molecular weight of the compound.
The g/L has been the mass of solute present in a L of solution. The g/L has the unit for density.
Molarity has been the moles of solute present in the liter of solution. It has been given as mol/L.
The product of g/mol and g/L gives the value of mol/L. Thus, to convert g/mol to g/L molarity can be used. Thus, option C is correct.
For more information about g/L refer to the link:
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Explain with examples following characteristics of chemical reactions: a. Change of colour b. Evolution of gas c. Change of smell d. Change of state
Answer:
Explanation:
a. change of colour:
A chemical reaction rearranges the constituent atoms of the reactants to create different substances as products. The products have different molecular structures than the reactants. Different atoms and molecules radiate different colours of light. Hence, there usually is a change in colour during a chemical reaction.
Eg: copper reactions with the elements
b. Evolution of gas:
A gas evolution reaction is a chemical reaction in which one of the end products is a gas such as oxygen or carbon dioxide.
Eg: ammonium hydroxide breaks down to water and ammonia gas.
c. Change of smell :
Production of an Odor Some chemical changes produce new smells. ... The formation of gas bubbles is another indicator that a chemical change may have occured.
Eg: The chemical change that occurs when an egg is rotting produces the smell of sulfur.
d. Change of state:
A chemical reaction is a process in which one or more substances, also called reactants, are converted to one or more different substances, known as products.
Eg: candle wax (solid) melts initially to produce molten wax (liquid)
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A silver cube with an edge length of 2.42 cm and a gold cube with an edge length of 2.75 cm are both heated to 85.4 ∘C and placed in 112.0 mL of water at 20.5 ∘C . What is the final temperature of the water when thermal equilibrium is reached?
Answer:
Explanation:
Volume of silver cube = 2.42³ = 14.17 cm³
mass of silver cube = volume x density
= 14.17 x 10.49 = 148.64 gm
Volume of gold cube = 2.75³ = 20.8 cm³
mass of gold cube = 20.8 x 19.3 = 401.44 gm
specific heat of silver and gold are .24 and .129 J /g°C
mass of 112 mL water = 112 g
Heat absorbed = heat lost = mass x specific heat x temperature fall or rise
Heat lost by metals
= 148.64 x .24 x ( 85.4 -T) + 401.44 x .129 x ( 85.4 - T )
= (35.67 + 51.78 ) x ( 85.4 - T )
87.45 x ( 85.4 - T )
= 7468.23 - 87.45 T
Heat gained by water
= 112 x 1 x ( T - 20.5 )
= 112 T - 2296
Heat lost = heat gained
7468.23 - 87.45 T = 112 T - 2296
199.45 T = 9764.23
T = 48.95° C
Consider the following reaction: C2H4(g)+H2(g)→C2H6(g) ΔH=−137.5kJ; ΔS=−120.5J/K Calculate ΔG at 25 ∘C and determine whether the reaction is spontaneous. Express the free energy change in joules to four significant figures.
Answer:
* [tex]\Delta G=-101.6kJ[/tex]
* Spontaneous reaction.
Explanation:
Hello,
In this case, for the given reaction, we can compute the Gibbs free energy by using the shown below equation:
[tex]\Delta G=\Delta H-T\Delta S[/tex]
In such a way, we proceed as follows with the proper units:
[tex]\Delta G=-137.5kJ-(25+273.15)K*(-120.5\frac{J}{K}*\frac{1kJ}{1000J} )\\\\\Delta G=-101.6kJ[/tex]
Therefore, since the Gibbs free energy of reaction is less than 0, the reaction is said to be spontaneous.
Best regards.
The value of ΔG should be -101.6KJ.
The reaction should be Spontaneous.
Calculation of the value of ΔG and reaction:Here the Gibbs free energy by using the below equation:
So,
=-137.5K - (25 + 273.15)K * (-120.5J/K * 1KH/1000J)
= -101.6KJ
As we can see that the Gibbs free energy of reaction is less than 0, the reaction is said to be spontaneous.
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what is the value of the equilibrium constant at 500k for a chemical equilivrium that has a delta h value of 250kj mol and s value of 48 j mol k
Match the words in the below to the appropriate blanks in the sentences.
1. When comparing the two elements A s and S n , the more metallic element is ______based on periodic trends alone.
2. When comparing the two elements G e and S b , the more metallic element is ________ based on periodic trends alone.
A. Ge
B. Pb
C. Sb
D. impossible to determine
E. K
Answer:
Sn and Ge
Explanation:
To obtain the more metallic element, we compare the group in which both elements are. Generally the element with the lower ionzation energy is he more metallic one.
Ionization energy increases fro left to right across a period. Ionization energy decreases down the group.
1. When comparing the two elements A s and S n , the more metallic element is ______based on periodic trends alone.
Sn has a lower ionization energy so it is the more metallic one.
2. When comparing the two elements G e and S b , the more metallic element is ________ based on periodic trends alone.
Ge has a lower ionizaiton energy compared to Sb. So it is more metallic element than Sb.
A sample of oxygen is collected over water at a total pressure of 692.2 mmHg at 17°C. The vapor pressure of water at 17°C is 14.5 mmHg. The partial pressure of the O2
Answer:
677.7 mmHg
Explanation:
The first empirical study on the behaviour of a mixture of gases was carried out by John Dalton. He established the effects of mixing gases at different pressures in the same vessel.
Dalton's law states that,the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the individual gases present in the mixture of gases. When a gas is collected over water, the gas also contains some water vapour. The partial pressure of the gas will now be given as; total pressure of gas mixture - saturated vapour pressure of water (SVP) at that temperature.
Given that;
Total pressure of gas mixture = 692.2 mmHg
SVP of water at 17°C = 14.5 mmHg
Therefore, partial pressure of oxygen = 692.2-14.5
Partial pressure of oxygen = 677.7 mmHg
Kinetic energy and gravitational potential energy are both forms of which type
of energy?
A. Internal energy
B. Mechanical energy
C. Potential energy
D. Thermal energy
Answer:
C. Potential energy
Explanation:
Kinetic energy and gravitational potential energy are both forms of potential energy. Potential energy is stored energy, when an object is not in motion it has stored energy. When an object is an motion it has kinetic energy. An object posses gravitational potential energy when it is above or below the zero height.
4. A puddle of coastal seawater, caught in a depression formed by some coastal rocks at high tide, begins to evaporate as the tide goes out. If the volume of a puddle decreases to 23% of its original volume, what is the sodium chloride concentration if it was initially 0.449 M?
Answer:
0.583M NaCl
Explanation:
Molarity is an unit of concentration defined as the ratio between moles of solute and liters of solution.
In the puddle, the solute is sodium chloride that is dissolved in water and you have 0.449 moles of NaCl per liter of water
When the solution begins to evaporate, amount of water decreases whereas moles of NaCl remain constant.
As 23% of the water evaporates, amount of water that remains is 100-23 = 77%, that means now you have 0.449 moles of NaCl per 77% of a liter, 0.770L. The new concentration is:
0.449 moles NaCl / 0.770L =
0.583M NaClAccording to solubility rules, which of the following compounds is insoluble in water?
A.Cal
2
B.NA SO
2 4
C.AgF
D.AI(OH)
3
Answer:
The correct answer is - Al(OH)3
Explanation:
At the point when a substance is blended in with a soluble, there are a few potential outcomes. The deciding variable for the outcome is the solubility of the substance, which is characterized as the maximum concentration of the solute. These rules help figure out which substances are solvent, and how much.
According to the 11 rules of solubility rules, the insoluble compound in water is - Al(OH)3
Answer:
Na2So4
Explanation:
If you consult a table of solubility rules, like the one below, you will see that sodium sulfate (Na2SO4) is soluble in water.
what bonding is similar to ionic bonding, except there are no high-electronegativity atosms present to accept any electrons that the present atoms are willing to donate.
Answer:
Metallic bonding
Explanation:
Ionic bonding involves the transfer of electrons from a highly electropositive metal to a highly electronegative nonmetal.
The metallic bond is somewhat similar to the ionic bond since there are also charged positive metal ions. The only difference is that there isn't any electronegative element that accepts the electrons.
In a metallic bond, the positively charged metal ions are bound together by a sea of mobile electrons. The attractive force between the metal ions and the mobile electrons hold the metallic crystal lattice together.
Cual es la diferencia entre agua pesada y agua ligera a) el agua pesada contiene mas minerales que el agua ligera b) el agua ligera es liquida mientras el agua pesada es solida c) el agua ligera es agua purificada y el agua pesada es agua contaminada d) el agua pesada contiene mas elementos estearato de sodio
Answer:
d) El agua pesada contiene mas elementos
Explanation:
La diferencia fundamental entre el agua pesada y el agua ligera es que la primera tiene una proporción mayor de deuterio que la segunda. El deuterio es un ión del hidrógeno que tiene un peso atómico mayor que el hidrógeno común y corriente. Por ende, la opción D ofrece la mejor aproximación.
Answer:
....................
lllllllllllllllll
Explanation:ki
a soluation of acetone in water has a molarity of 2.422M and a density of 0.970 g/mL. Calculate the mole fraction
Answer:
[tex]x_{acetone}=7.970x10^{-3}[/tex]
Explanation:
Hello,
In this case, for the given molarity, we can assume a volume of 1 L of solution, to obtain the following moles of acetone:
[tex]n=0.422mol/L*1L=0.422mol[/tex]
Then, with the density of solution, we can compute the mass of the solution for the selected 1-L volume basis:
[tex]m_{solution}=1L*\frac{1000mL}{1L}*\frac{0.970g}{1mL}=970g[/tex]
After that, we compute the mass of water in the solution, considering the mass of acetone (molar mass = 58.08 g/mol):
[tex]m_{H_2O}=970g-0.422molAcetone*\frac{58.08g\ Acetone}{1mol\ Acetone} =945.49gH_2O[/tex]
Next, the moles of water:
[tex]n_{H_2O}=945.49g*\frac{1molH_2O}{18gH_2O} =52.53molH_2O[/tex]
Finally, the mole fraction:
[tex]x_{acetone}=\frac{n_{acetone}}{n_{acetone}+n_{H_2O}}=\frac{0.422mol}{0.422mol+52.53mol}\\ \\x_{acetone}=7.970x10^{-3}[/tex]
Regards.
What are the correct formulas and coefficients for the products of the following double-replacement reaction? RbOH + H3PO4→
Answer:
3 RbOH + H₃PO₄ → Rb₃PO₄ + 3 H₂O
Explanation:
Let's consider the double-replacement reaction between rubidium hydroxide and phosphoric acid to form rubidium phosphate and water. The cation rubidium replaces the cation hydrogen and the anion hydroxyl replaces the anion phosphate. The balanced chemical reaction is:
3 RbOH + H₃PO₄ → Rb₃PO₄ + 3 H₂O