Answer:
HCl
Explanation:
Choices:
CO: 28.01g/mol
NO₂: 46g/mol
CH₄: 16.04g/mol
HCl: 36.4g/mol
CO₂: 44.01g/mol
It is possible to identify a substance finding its molar mass (That is, the ratio between its mass in grams and its moles). It is possible to find the moles of the gas using general ideal gas law:
PV = nRT
Where P is pressure of gas 0.764atm; V its volume, 0.279L; n moles; R gas constant: 0.082atmL/molK and T its absolute temperature, 295.85K (22.7°C + 273.15).
Replacing:
PV = nRT
PV / RT = n
0.764atm*0.279L / 0.082atmL/molKₓ295.85K = n
8.786x10⁻³ = moles of the gas
As the mass of the gas is 0.320g; its molar mass is:
0.320g / 8.786x10⁻³moles = 36.4 g/mol
Based in the group of answer choices, the identity of the gas is:
HCl
Molar mass of substance is the mass of one mole of substance. The gas is identified as HCl as it has 36.4 g/mol of molar mass.
The substance can be identified from its molar mass. The formula to calculate the molar mass is
[tex]\bold {m = \dfrac w{n}}[/tex]
Where,
n - number of moles
w - given mass of the substance
The number of moles can be calculated by the using ideal gas law
PV = nRT
[tex]\bold {n = \dfrac {PV }{ RT }}[/tex]
Where
P - pressure of gas 0.764 atm;
V its volume, 0.279 L;
n moles;
R gas constant: 0.082atmL/molK
T its absolute temperature, 295.85 K (22.7°C + 273.15).
Put the values in the formula,
[tex]\bold {n = \dfrac {0.764\ atm \times , 0.279 }{ 0.082 \times 295.85 }}\\\\\bold {n =8.786x10^-^3}[/tex]
Now, put the values in the molar mass formula,
[tex]\bold {m = \dfrac {0.320g}{ 8.786x10^-^3} = 36.4\ g/mol}[/tex]
Therefore, the gas is identified as HCl as it has 36.4 g/mol of molar mass.
To know more about molar mass,
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A mixture with H2 and He exerts a total pressure of 0.48 atm. If there is 1.0 g of H2 and 1.0 g of He in the mixture, what is the partial pressure (in atmospheres) of hydrogen?
Answer:
Partial pressure of hydrogen H₂ = 0.32 atm
Explanation:
Given:
Total pressure = 0.48 atm
Find:
Partial pressure of hydrogen
Computation:
Number of mole of H₂ = 1 / 2 = 0.5 moles
Number of mole of He = 1 / 4 = 0.25 moles
Total moles = 0.5 + 0.25 = 0.75
Partial pressure of hydrogen H₂ = [moles / total moles] Total pressure
Partial pressure of hydrogen H₂ = [0.50 / 0.75]0.48 atm
Partial pressure of hydrogen H₂ = 0.32 atm
Answer: 0.32 atm
Explanation:
First convert the mass of H2 to moles using the molar mass.
(1.0 gram H2 ⋅ (1.0 mol H2 / 2.016 g H2)) ≈ 0.50 mol H2
Next, convert the mass of helium He to moles using the atomic mass.
(1.0 gram He ⋅ (1.0 mol He / 4.003 g He)) ≈ 0.25mol He
The total number of moles is about 0.75 moles . The partial pressure of a component of a gas mixture can be found by multiplying the mole fraction by the total pressure.
PH2 = XH2 × Ptotal
PH2 = (0.50 mol / 0.75 mol)(0.48 atm) = 0.32 atm
Which of the following aqueous solutions are good buffer systems? . a. 0.12 M calcium hydroxide + 0.29 M calcium bromide . b. 0.25 M perchloric acid + 0.16 M sodium perchlorate . c. 0.34 M hydrocyanic acid + 0.27 M sodium cyanide .
Answer:
c. 0.34 M hydrocyanic acid + 0.27 M sodium cyanide .
Explanation:
A buffer is defined as the aqueous mixture of a weak acid with its conjugate base or vice versa. Based on the systems:
a. 0.12 M calcium hydroxide + 0.29 M calcium bromide. IS NOT A GOOD BUFFER SYSTEM because Ca(OH)₂ is a strong base.
b. 0.25 M perchloric acid + 0.16 M sodium perchlorate. IS NOT A GOOD BUFFER SYSTEM because perchloric acid is a strong acid
c. 0.34 M hydrocyanic acid + 0.27 M sodium cyanide. IS A GOOD BUFFER SYSTEM because HCN is a weak acid, and its conjugate base, CN⁻, is obtained in the dissolution of NaCN as Na⁺ and CN⁻ ions.
When a hydrochloric acid solution is combined with a potassium hydroxide solution, an acid-base reaction occurs Write a balanced molecular equation for this reaction. Express your answer as a chemical equation. Identify all of the phases in your answer..
Answer:
HCl(aq) + KOH(aq) ⇒ KCl(aq) + H₂O(l)
Explanation:
Hydrochloric acid is an acid because it releases H⁺ in an aqueous solution.
Potassium hydroxide is a base because it releases OH⁻ in an aqueous solution.
When an acid reacts with a base they form a salt and water. This is a neutralization reaction. The neutralization reaction between hydrochloric acid and potassium hydroxide is:
HCl(aq) + KOH(aq) ⇒ KCl(aq) + H₂O(l)
Average Molarity for HCl is .391
Average Molarity for NaOH is .0962
Volume for HCl is:
Trial 1 Your Answer: 14mL
Trial 2 Your Answer: 14mL
Trial 3 Your Answer: 14mL
Volume for NaOH is:
Trial 1: 34.26mL
Trial 2: 33.48mL
Trial 3: 33.84mL
Entry # mass tablet(g) mass antacid(g) Vol HCl(mL) Vol NaOH(mL)
#1: 1.515 0.9010 14.00 34.26
#2: 1.452 0.8370 14.00 33.48
#3: 1.443 0.8280 14.00 33.84
I need help finding the mmoles HCl/mg please.
Answer:
#1: 0.00144 mmolHCl/mg Sample
#2: 0.00155 mmolHCl/mg Sample
#3: 0.00153 mmolHCl/mg Sample
Explanation:
A antiacid (weak base) will react with the HCl thus:
Antiacid + HCl → Water + Salt.
In the titration of antiacid, the strong acid (HCl) is added in excess, and you're titrating with NaOH moles of HCl that doesn't react.
Moles that react are the difference between mmoles of HCl - mmoles NaOH added (mmoles are Molarity×mL added). Thus:
Trial 1: 0.391M×14.00mL - 0.0962M×34.26mL = 2.178 mmoles HCl
Trial 2: 0.391M×14.00mL - 0.0962M×33.48mL = 2.253 mmoles HCl
Trial 3: 0.391M×14.00mL - 0.0962M×33.84mL = 2.219 mmoles HCl
The mass of tablet in mg in the 3 experiments is 1515mg, 1452mg and 1443mg.
Thus, mmoles HCl /mg OF SAMPLE for each trial is:
#1: 2.178mmol / 1515mg
#2: 2.253mmol / 1452mg
#3: 2.219mmol / 1443mg
#1: 0.00144 mmolHCl/mg Sample#2: 0.00155 mmolHCl/mg Sample#3: 0.00153 mmolHCl/mg SampleAl(NO3)3+H2SO4=HNO3+Al2(SO4)3
Hey there!:
2 Al(NO)₃+ 3 H₂SO₄ → 1 Al₂O₁₂S₃+ 6 HNO₃
Reagents : Al(NO₃)₃ and H₂SO₄
Products : Al₂O₁₂S₃ and HNO₃
Coefficients : 2 , 3 , 1 and 6
Hope this helps!
Each energy sub level contains __________ number of electrons. For example, sub level D can hold up to _______ electrons. A. the same, 10 B. the same, 14 C. a different, 6 D. a different, 10
Answer:
the same and 14
Explanation:
ed tell chem
Answer: the same 10
Explanation:
Which of the possible compounds has a mass of 163 grams when
6.13 x 1024 molecules of the compound is put on a scale?
Answer:
CH4
Explanation:
In solving this problem, we must remember that one mole of a compound contains Avogadro's number of elementary entities. These elementary entities include atoms, molecules, ions etc. Recall that one mole of a substance is the amount of substance that contains the same number of elementary entities as 12g of carbon-12. The Avogadro's number is 6.02 × 10^23.
Hence we can now say;
If 163 g of the compound contains 6.13 ×10^24 molecules
x g will contain 6.02 × 10^23 molecules
x= 163 × 6.02 × 10^23 / 6.13 × 10^24
x= 981.26 × 10^23/ 6.13 ×10^24
x= 160.1 × 10^-1 g
x= 16.01 g
x= 16 g(approximately)
16 g is the molecular mass of methane hence x must be methane (CH4)
solution solution solution
Answer:
Oxygen present in food items makes then rancid due to the presence of oils and fats. If the food is flushed with nitrogen, it prevents it from being oxidised (the nitrogen acts as an antioxidant).
Hope it helps ! :)
Which aqueous solution will have the highest boiling point temperature? A. 0.100 molal NiBr2(aq) B. 0.250 molal CH3OH(aq) C. 0.100 molal MgSO4(aq) D. 0.150 molal Na2SO4(aq) E. 0.150 molal NH4NO3(aq)
Answer: 0.150 m [tex]Na_2SO_4(aq)[/tex] will have highest boiling point.
Explanation:
Formula used for Elevation in boiling point :
[tex]\Delta T_b=i\times k_b\times m[/tex]
where
[tex]\Delta T_b=T_b-T^o_b[/tex]= elevation in boiling point
[tex[k_b[/tex] = boiling point constant
m = molality
i = Van't Hoff factor
A) 0.100 m [tex]NiBr_2[/tex]
i = 3 as [tex]NiBr_2\rightarrrow Ni^{2+}+2Br^-[/tex]
concentration will be [tex]3\times 0.100=0.300[/tex]
B) 0.250 m [tex]CH_3OH[/tex]
i = 1 as [tex]CH_3OH[/tex] is a non electrolyte
concentration will be [tex]1\times 0.250=0.250[/tex]
C) 0.100 molal [tex]MgSO_4(aq)[/tex]
i = 2 as [tex]MgSO_4\rightarrrow Mg^{2+}+SO_4^{2-}[/tex]
concentration will be [tex]2\times 0.100=0.200[/tex]
D. 0.150 molal [tex]Na_2SO_4(aq)[/tex]
i = 3 as [tex]Na_2SO_4\rightarrrow 2Na^{+}+SO_4^{2-}[/tex]
concentration will be [tex]3\times 0.150=0.450[/tex]
E. 0.150 molal [tex]NH_4NO_3(aq)[/tex]
i = 2 as [tex]NH_4NO_3\rightarrrow NH_4^{+}+NO_3^{-}[/tex]
concentration will be [tex]2\times 0.150=0.300[/tex]
The solution having the highest concentration of ions will have the highest boiling point and thus 0.150 m [tex]Na_2SO_4(aq)[/tex] will have highest boiling point.
The aqueous solution that would have the highest temperature at boiling point would be:
D). 0.150 molal Na2SO4(aq)
What is a boiling point?The boiling point is described as the temperature at which the solution starts boiling or the vapor pressure becomes equivalent to the provided external/outer pressure.
To determine the elevation in boiling point, we will use:
Δ[tex]T_{b}[/tex] [tex]= i[/tex] × [tex]k_{b}[/tex] × [tex]m[/tex]
with
[tex]T_{b}[/tex] [tex]= T_{b} - T^{0}_{b}[/tex]
[tex]k_b[/tex] [tex]=[/tex] constant of boiling point
Using this formula,
0.150 molal Na2SO4(aq)
Given,
[tex]i = 3[/tex]
[tex]Na2So4[/tex] will have
[tex]2Na^{+}[/tex] [tex]+[/tex] [tex]SO^{2-}_{4}[/tex]
So,
Concentration [tex]= 3[/tex] × [tex]0.15[/tex][tex]0[/tex]
[tex]= 0.45[/tex][tex]0[/tex]
∵ 0.150 molal [tex]Na2SO4[/tex]Na2SO4(aq) has the maximum concentration.
Thus, option D is the correct answer.
Learn more about "Aqueous solution" here:
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(4Ga + 3S2 → 2Ga2S3)
1. How many moles of Sulfur are needed to react with 12.5 moles of Gallium
Answer:
9.375
Explanation:
According to the chemical equation, for every 4 moles of gallium, 3 moles of sodium are needed to react. Set up a ratio using this relationship to solve.
4/3 = 12.5/x
4x = 37.5
x = 9.375
You need 9.375 moles of sulfur.
According to valence bond theory, which orbitals overlap in the formation of the bond in HCl?
a) 1s on H and 3p on Cl
b) 1s on H and 4s on Cl
c) 1s on H and 2p on Cl
d) 2s on H and 3p on Cl
e) 2s on H and 2p on Cl
If the NaOH is added to 35.0 mL of 0.167 M Cu(NO3)2 and the precipitate isolated by filtration, what is the theoretical yield of the reaction?
Answer:
The correct answer is - 0.570 grams
Explanation:
The balanced chemical reaction is given by
Cu(NO3)2(aq) + 2NaOH(aq) --------> Cu(OH)2(s) + 2NaNO3(aq)
1.0 mole 2.0 mole 1.0 mole 2.0 mole
number of mol of Cu(OH)2,
n = Molarity * Volume
= [tex]35.0*0.167 = 5.845[/tex] millimoles
As clear in the equation, 1 mole of Cu(NO3)2 gives 1 mole of Cu(OH)2 , So, 5.845 millimoles of Cu(NO3)2 will produce 5.845 millimoles of Cu(OH)2
Mass of Cu(OH)2 = number of mol * molar mass
= [tex]97.5*5.845*10^-3[/tex]
= 0.570 grams
Thus, the correct answer is - 0.570 grams
A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. A buffer region was found around a pH of 3.5. The unknown compound is
Answer:
The unknown compound is a weak acid.
Explanation:
Given that :
a 25 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution.
A buffer region was found around a pH of 3.5. We know that a pH of 3.5 is a weak acid. So, it is likely to be an organic acid
Let assume the solution of the unknown sample to be CH₃COOH
Now :
25 mL of CH₃COOH reacted with 0.115 M of NaOH
The equation for the reaction will be :
CH₃COOH + NaOH -----> CH₃COONa + H₂O
at x mole of 0.115y M of
CH₃COOH NaOH is present
If NaOH was added in excess;
CH₃COOH + NaOH -----> CH₃COONa , NaOH will be lost then CH₃COOH and CH₃COONa will be present
Therefore;
At equilibrium : Only CH₃COONa will be present but if it is above equilibrium NaOH will be present because the pH will increase due to the presence of the strong base
Determine the enthalpy change when 19.399999999999999 g of carbon is reacted with oxygen according to the reaction
Answer:
The enthalpy change is −636.9798 kJ
Explanation:
The equation of the reaction between Carbon and Oxygen can be represented as :
[tex]C_{(s)} + O_{2(g)} \to CO_{2_(g)} \ \ \ \ \ \ \Delta H = -394 \ \ kJ/mol[/tex]
molar mass of Carbon = 12 mole
when mass of 19.399999999999999 g of carbon reacted with oxygen;
the number of moles = mass/molar mass
the number of moles = 19.399999999999999/12
the number of moles = 1.6167 mol
Thus the enthalpy change when 1 mole of carbon react with oxygen = -394 kJ/mol
Therefore when 1.6167 moles react with oxygen; we have:
= 1.6167 mol × -394 kJ/mol
= −636.9798 kJ
A metal, M , of atomic mass 56 amu reacts with chlorine to form a salt that can be represented as MClx. A boiling point elevation experiment is performed to determine the subscript x , and therefore, the formula of the salt. A 22.9 g sample of the salt is dissolved in 100.0 g of water and the boiling point of the solution is found to be 375.93 K. Find the formula of the salt. Assume complete dissociation of the salt in solution g
Answer:
Formula for the salt: MCl₃
Explanation:
MClₓ → M⁺ + xCl⁻
We apply the colligative property of boiliing point elevation.
We convert the boiling T° to °C
375.93 K - 273K = 102.93°C
ΔT = Kb . m . i
where ΔT means the difference of temperature, Keb, the ebulloscopic constant for water, m the molality of solution (mol of solute/kg of solvent) and i, the Van't Hoff factor (numbers of ions dissolved)
ΔT = 102.93°C - 100°C = 2.93°C
Kb = 0.512 °C/m
We replace data: 2.93°C = 0.512 °C/m . m . i
i = x + 1 (according to the equation)
22.9 g / (56g/m + 35.45x) = moles of salt / 0.1kg = molality
We have calculated the moles of salt in order to determine the molar mass, cause we do not have the data. We replace
2.93°C = 0.512 °C/m . [22.9 g / (56g/m + 35.45x)] / 0.1kg . (x+1)
2.93°C / 0.512 m/°C = [22.9 g / (56g/m + 35.45x)] / 0.1kg . (x+1)
5.72 m = [22.9 g / (56g/m + 35.45x)]/ 0.1 (x+1)
5.72 . 0.1 / [22.9 g / (56g/m + 35.45x)] = x+1
0.572 / (22.9 g / (56g/m + 35.45x) = x+1
0.572 (56 + 35.45x) / 22.9 = x+1
0.572 (56 + 35.45x) = 22.9x + 22.9
32.03 + 20.27x = 22.9x + 22.9
9.13 = 2.62x
x = 3.48 ≅ 3
What is the mass of 7.68 x 1024 molecules of phosphorus trichloride?
Answer:
THE MASS OF 7.68 *10^24 MOLECULES OF PHOSPHORUS TRICHLORIDE IS 1746.25 g.
Explanation:
Molar mass of PCl3 = ( 31 + 35.5 *3) = 137.5 g/mol
At 7.68 * 10^24 molecules, how many number of mole is present?
6.03 * 10^23 molecules = 1 mole
7.68*10^24 molecules = x mole
x mole = 7.68 *10^24 molecules/ 6.03 *10^23
x mole = 1.27 *10 moles
x mole = 12.7 moles
Using mole = mass / molar mass
mass = mole * molar mass
mass = 12.7 moles * 137.5 g/mol
mass = 1746.25 g
Hence, the mass of 7.68 *10^24 molecules is 1746.25 g
In the naturally occurring D series of ketoses, the carbonyl group is found on carbon number ___________, whereas in aldoses, the carbonyl group is found on carbon number _________.
Answer:
second carbon atom from the end
end carbon atom
Explanation:
Carbohydrates are naturally occurring organic compounds containing carbon, hydrogen and oxygen. The general molecular formula of Carbohydrates is [tex]C_x(H_2O)_y[/tex].
Carbohydrates can be classified based on structures,
Carbohydrates with the structure of alkanals (-CHO) are known as aldose while those of the structure of alkanones (C=O) are known as ketose.
In stereochemistry , D series is a kind of configurational arrangement where the hydroxyl group attaches itself to the right hand side.
Thus; in naturally occurring D series of ketoses, the carbonyl group is found on carbon number second carbon atom from the end whereas in aldoses, the carbonyl group is found on carbon number end carbon atom.
Calculate the amount of heat required to convert 10.0 grams of ice at –20.°C to steam at 120.°C. (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O(l) = 4.18 J/g•°C, Sp. heat of H2O(gas) = 2.03 J/g•°C; heat of fusion of H2O(solid) = 333 J/g, heat of vaporization of H2O(liquid) = 2260 J/g).
Answer:
THE AMOUNT OF HEAT REQUIRED TO CONVERT ICE FROM -20 C TO STEAM AT 120 C IS 30 946 J OR 30.946 KJ OF HEAT.
Explanation:
Mass = 10 g
To convert 10 g of ice at -20°C to steam at 120°C, the heat involved is:
1. Heat involved in converting the ice from -20 °c to ice at 0 °C:
Heat = mass * specific heat of water solid * change in temperature
heat = 10g * 2.09 J/g°C * ( 0- (-20))
Heat = 10 * 2.09 * 20
heat = 418 J
2. Heat required to convert the ice from 0°C to water at 0°C:
Heat = mass * specific heat of fusion of water solid
Heat = 10 * 333
Heat = 3330 J
3. Heat required to convert water at 0 C to water at 100 C:
Heat = mass * specific heat of water * change in teperature
Heat = 10 * 4.18 * (100 -0)
Heat = 4180 J
4. Heat required to convert water at 100 C to steam at 100 C:
Heat = mass * specific heat of vaporization
Heat = 10 * 2260
Heat = 22600 J
5. Heat required to convert steam from 100 C to steam at 120 C:
Heat = mass * specific heat of water * change in temperature
Heat = 10 * 2.09 * (120 -100)
Heat = 10 * 2.09 * 20
Heat = 418 J
T
he heat required to convert 10 g of ice at -20 C to steam at 120 C is therefore the total of the individual heat of reactions
Total amount of heat = ( 418 J + 3330 J + 4180 J + 22600 J + 418 J)
Total heat = 30946 J
Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation:
PCl5(g) = PCl3(g) + Cl2(gu)
at 250 Co , 0.125M PCl5 is added to the flask , if Kc=1.80, what are the equilibrium concentrations of each gas?
A) [PCl5]=0.0625M,[PCl3]=0.0335M,and [Cl2]=0.335M
B) [PCl5]=1.80M,[PCl3]=1.80M,and [Cl2]=1.80M
C) [PCl5]=0 M,[PCl3]=1.34M,and [Cl2]=1.34M
D) [PCl5]=0.00765M,[PCl3]=0.117M,and [Cl2]=0.0.117M
E) [PCl5]=3.96M,[PCl3]=3.83M,and [Cl2]=3.83M
Answer:
D) [PCl5]=0.00765M,[PCl3]=0.117M,and [Cl2]=0.0.117M
Explanation:
Based on the reaction:
PCl₅(g) ⇄ PCl₃(g) + Cl₂(g)
And knowing:
Kc = [PCl₃] [Cl₂] / [PCl₅] = 1.80
When you add PCl₅ into a flask, this gas will react producing PCl₃ and Cl₂ until [PCl₃] [Cl₂] / [PCl₅] = 1.80
This could be written as:
[PCl₃] = X
[Cl₂] = X
[PCl₅] = 0.125M - X
Where X represents the moles of PCl₅ that react, reaction coordinate.
Replacing in Kc expression:
[PCl₃] [Cl₂] / [PCl₅] = 1.80
[X [X] / [0.125 - X] = 1.80
X² = 0.225 - 1.80X
0 = -X² -1.80X + 0.225
Solving for X:
X = -1.9M → False solution, there is no negative concentrations
X = 0.11735M → Right solution.
Replacing, concentrations in equilibrium are:
[PCl₃] = X
[Cl₂] = X
[PCl₅] = 0.125M - X
[PCl₃] = 0.117M
[Cl₂] = 0.117M
[PCl₅] = 0.00765M
And right option is:
D) [PCl5]=0.00765M,[PCl3]=0.117M,and [Cl2]=0.0.117MSuppose you are working with a NaOH stock solution but you need a solution with a lower concentration for your experiment. Calculate the volume (in milliliters) of the 1.436 M stock NaOH solution needed to prepare 250.0 mL of 0.1342 M dilute NaOH solution.
Answer:
23.36mL of the stock solution are required.
Explanation:
A dilution consist in the addition of solvent to decreases the concentration of a stock solution (The solution more concentrated).
As you want to prepare 250.0mL = 0.2500L of a 0.1342M NaOH, moles of NaOH you require to make this concentration in this volume are:
0.2500L × (0.1342mol / L) = 0.03355 moles of NaOH you require in the diluted solution.
These moles comes from the 1.436M stock solution. The volume of the stock solution you need to add is:
0.03355moles NaOH × (1L / 1.436mol) = 0.02336L of the 1.436M solution =
23.36mL of the stock solution are required.A 32.3-gram sample of gas is found to have a volume of 1.9 liters at 301 K and 1.21 atm. What is the molar mass of this gas? Show all of the work used to solve this problem.
Answer:
351.1g/mol
Explanation:
you can find the answer using The ideal gas equation
n= PV/RT
n=(1.21*1.9/0.082*301)mol
n=0.092 mol
molar mass=Mass/mole
m=32.3g/0.092mol
m=351.1g/mol
Describe what happens when two substances at different temperatures cine into contact. Describe how the law of conservation of energy applies to this system
Answer:
The substance with the highest heat gives heat to the lowest temperature, equating both temperatures,
In this situation there is talk of giving up heat but not matter, it is here that the law of conservation of energy comes into play.
Explanation:
The law of conservation of energy talks about that energy is transformed and never lost between two substances or two bodies that interact with each other, these interactions can be heat exchanges, as in this example.
4. What is the molar concentration and grams/Liter of a NaOH solution if 86 ml are titrated to an
endpoint by 375 ml of a solution of HCl that is .0175 M?
g/L: ________
Molarity: ____
Answer:
0.76 M
30 g/L
Explanation:
Step 1: Given data
Molarity of the acid (Ma): 0.175 MVolume of the acid (Va): 375 mLMolarity of the base (Mb): ?Volume of the base (Vb): 86 mLStep 2: Calculate the molarity of the base
We will use the following expression.
[tex]Ma \times Va = Mb \times Vb\\Mb = \frac{Ma \times Va}{Vb} = \frac{0.175M \times 375mL}{86mL} = 0.76 M[/tex]
Step 3: Calculate the concentration of the base in g/L
The molar mass of NaOH is 40.00 g/mol.
[tex]\frac{0.76mol}{L} \times \frac{40.00g}{mol} = 30 g/L[/tex]
can somebody please help me asap !!!
Answer:
Option A. 1191.49 K
Explanation:
Data obtained from the question include:
The equation for the reaction is given below:
4HCl + O2 —> 2Cl2 + 2H2O
Enthalpy (H) = +280 KJ/mol = +280000 J/mol
Entropy (S) = +235 J/Kmol
Temperature (T) =..?
The temperature at which the reaction will be feasible can be obtained as follow:
Change in entropy (ΔS) = change in enthalphy (ΔH)/T
(ΔS) = (ΔH)/T
235 = 280000/T
Cross multiply
235 x T = 280000
Divide both side by 235
T = 280000/235
T = 1191.49 K
Therefore, the temperature at which the reaction will be feasible is 1191.49 K
Grams of cl in 38g of cf3cl
Answer:
114 grams
Explanation:
3chlorines per compound*38grams=114
If the reaction consumes methane gas ( CH4 ) at a rate of 2.08 M/s, what is the rate of formation of H2 ? the balanced equation is CH4 + N2Cl4 = CCl4 + N2 + 2 H2
Answer:
4.16M/s
Explanation:
Based on the reaction:
CH₄ + N₂Cl₄ ⇄ CCl₄ + N₂ + 2H₂
1 mole of methane, CH₄, produce 2 moles of H₂.
That means whereas 1 mole of methane is consumed, 2 moles of H₂ are formed
Having this in mind, if you are consuming methane at a rate of 2.08M/s, the rate of formation of hydrogen must be twice this rate, because there are produced twice moles of H₂.
Thus, rate of formation of H₂ is:
2.08M/s ₓ 2 =
4.16M/s
The rate of formation of H2 is 4.16M/s
The calculation is as follows:Based on the reaction:
CH₄ + N₂Cl₄ ⇄ CCl₄ + N₂ + 2H₂
here
1 mole of methane, CH₄, produce 2 moles of H₂.
In the case when you are consuming methane at a rate of 2.08M/s, the rate of formation of hydrogen must be twice this rate, because there are produced twice moles of H₂.
Thus, rate of formation of H₂ is:
2.08M/s ( 2) = 4.16M/s
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For a given sample of C3H8(g), the enthalpy change during the reaction is -784kJ. How many grams of CO2 are produced? Group of answer choices g
Answer:
[tex]m_{CO_2}=46.6gCO_2[/tex]
Explanation:
Hello,
In this case, considering the combustion of propane:
[tex]C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(g)\ \ \ \Delta _CH=-2220.0 kJ/mol[/tex]
We can compute the burnt moles of propane as shown below:
[tex]n=\frac{-784kJ}{-2220.0 kJ/mol} =0.353molC_3H_8[/tex]
Then, by noticing propane and carbon dioxide are in a 1:3 molar ratio, we can compute the grams carbon dioxide by using the shown below stoichiometric procedure:
[tex]m_{CO_2}=0.353molC_3H_8*\frac{3molCO_2}{1molC_3H_8} *\frac{44gCO_2}{1molCO_2} \\\\m_{CO_2}=46.6gCO_2[/tex]
Best regards.
Why does a new period start on the periodic table, instead of the row continuing? A. A new period starts when a new energy shell starts. B. A new period starts when a new neutron cycle starts. C. None of these D. It is based on how many protons it has.
Answer:
B
Explanation:
All the elements in a period have valence electrons in the same shell. The number of valence electrons increases from left to right in the period. When the shell is full, a new row is started and the process repeats.
A new period starts when a new neutron cycle starts. Hence, option B is correct.
What is the period in the periodic table?A period in the periodic table is a row of chemical elements. All elements in a row have the same number of electron shells.
All the elements in a period have valence electrons in the same shell.
The number of valence electrons increases from left to right in the period.
When the shell is full, a new row is started and the process repeats.
Hence, option B is correct.
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A 2.0 g sample of hydrocarbon was burned in the calorimeter. The temperature rose from 29°c to 32°c and heat and combustion is 11. Kj/g. Thr heat capacity of the calorimeter is
Answer:
THE HEAT CAPACITY OF THE CALORIMETER IS 3666.67 J/C
Explanation:
Mass = 2 g
Temperature difference = 32 C - 29 C = 3 C
Heat of combustion = 11 kJ/g
Heat capacity of the calorimeter = unknown
It is important to note that the heat of combustion of the reaction is the heat absorbed by the calorimeter in raising the mixture by 3 C
So therefore,
Heat = heat capacity * temperature difference
Heat capacity = Heat / temperature difference
Heat capacoty = 11 000 J / 3 C
Heat capacity = 3666.67 J/ C
The graph below shows the half life values of parent isotopes
Based on the graph, it can be concluded that the isotope which is most likely to be found with 12.5% of its original amount in 42 billion years is
Answer:
Thorium-235
Explanation:
Half-life is defined as the time taken for a radioactive material to reduce to half of its original amount. If the original amount of a radioactive substance N is 100%, then;
1st half-life- 50% of N is left
2nd half life - 25% of N is left
3rd half-life- 12.5% of N is left
The half-life of Thorium-235 is 15 billion years, hence three half lives will take place in 45 billion years. Hence 12.5% of the original amount of Thorium-235 present will remain after about 42 billion years.