Answer:
B
Explanation:
What heats up faster but loses heat faster?
-Water
-Air
Or
Land
A student pours 800.0 mL of a 3.000 molar solution of sodium hydroxide into a 2.00 liter volumetric flask and fills the flask up with water. What is the new molarity of the solution?
A) 12.00 M
B) 1.20 M
C) 14.00 M
D) 0.0750 M
4NH3 + 502 --> 4NO + 6H20
How much excess reactant is leftover after if 6.30g of ammonia react with
1.80g of oxygen?
Answer:
5.52 g
Explanation:
4NH₃ + 5O₂ → 4NO + 6H₂OFirst we convert the given masses of both reactants into moles, using their respective molar masses:
6.30 g NH₃ ÷ 17 g/mol = 0.370 mol NH₃ 1.80 g O₂ ÷ 32 g/mol = 0.056 mol O₂Now we calculate with how many NH₃ moles would 0.056 O₂ moles react, using the stoichiometric coefficients:
0.056 mol O₂ * [tex]\frac{4molNH_3}{5molO_2}[/tex] = 0.045 mol NH₃As there more NH₃ moles than required, NH₃ is the excess reactant.
Then we calculate how many NH₃ moles remained without reacting:
0.370 mol NH₃ - 0.045 mol NH₃ = 0.325 mol NH₃Finally we convert NH₃ moles into grams:
0.325 mol NH₃ * 17 g/mol = 5.52 gHow do surface currents differ from deep ocean currents? Deepwater currents are dependent on the wind and landmasses. Deepwater currents are dependent on temperature and salinity. Deep ocean currents are affected by salinity and wind. None of the above
Answer:
surface currents are caused by winds : deep water currents are caused by difference in water density.
I guess the answer of your question is this
Answer:
Deepwater currents are dependent on temperature and salinity.
Explanation:
How much heat (in kJ) would need to be removed to cool 150.3 g of water from 25.60°C to -10.70°C?
Answer:
Q = -22.9 kJ
Explanation:
Given that,
Mass of water, m = 150.3 g
Water gets cool from 25.60°C to -10.70°C.
The specific heat of water, c = 4.2 J/g°C
The formula for heat needed is given by :
[tex]Q=mc\Delta T\\\\Q=150.3\times 4.2 \times (-10.7-25.6)\\\\Q=-22914.738\\\\or\\\\Q=22.9\ kJ[/tex]
So, 22.9 kJ of heat is needed to be removed to cool.
does water burn? for my sister that says water does burn
Answer:
No, water doesn't burn. It only can burn under specific conditions in a lab.
Explanation:
(giving brainiest) solve please! dont copy I've looked up everything ill know if you copied something!
Answer:
Precipitation falls in liquid and solid
Evaporation changes liquid water to gas
Explanation:
Precipitation exists in snow, rain, sleet, many forms liquid or solid but NOT gas.
Evaporation is from a liquid to a gas change, also called vaporization.
arrow futhermost to left is evaporation (rising into air)
arrow futhermost to right is precipitation ( falling back to ground)
hope this helped xxx please mark brainliest
During a titration, the pH of an analyte solution containing HA(aq) is 3.92 and the ratio of [A–]/[HA] is 0.41. What is the Ka of HA?
Answer:
[tex]Ka=4.71x10^{-4}[/tex]
Explanation:
Hello there!
In this case, according to the Henderson-Hasselbach equation, it is possible to write:
[tex]pH=pKa+log(\frac{[A^-]}{[HA]} )[/tex]
Next, since we are given the pH and the [A–]/[HA] ratio, we can solve for the pKa as shown below:
[tex]pKa=pH-log(\frac{[A^-]}{[HA]} )[/tex]
Now, we plug in the values to obtain:
[tex]pKa=3.92-log(0.41 )\\\\pKa=3.33[/tex]
Next, Ka is:
[tex]Ka=10^{-pKa}=10^{-3.33}\\\\Ka=4.71x10^{-4}[/tex]
Best regards!
For many purposes we can treat propane (CH) as an ideal gas at temperatures above its boiling point of - 42°C. Suppose the temperature of a sample of propane gas is lowered from 25.0°C to - 22.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.58 kPa and the volume decreased by 40.0%, what is the final pressure?
Answer: The final pressure is 0.81 kPa
Explanation:
The combined gas equation is,
[tex]\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}[/tex]
where,
[tex]P_1[/tex] = initial pressure of gas = 0.58 kPa
[tex]P_2[/tex] = final pressure of gas = ?
[tex]V_1[/tex] = initial volume of gas = v
[tex]V_2[/tex] = final volume of gas = [tex]v-\frac{40}{100}\times v=0.6v[/tex]
[tex]T_1[/tex] = initial temperature of gas = [tex]25^0C=(25+273)K=298K[/tex]
[tex]T_2[/tex] = final temperature of gas = [tex]-22^0C=(-22+273)K=251K[/tex]
Now put all the given values in the above equation, we get:
[tex]\frac{0.58\times v}{298}=\frac{P_2\times 0.6v}{251}[/tex]
[tex]P_2=0.81kPa[/tex]
The final pressure is 0.81 kPa
which has a higher ionization energy magnesium or calcium?
Answer:
magnesium has a higher ionization energy because its radius is smaller. calcium has a higher ionization energy because it outermost sub-energy level is full. they have the same ionization energy because they have the same number of valence electrons.
Explanation:
hope this helps
Identify each of the patterns labeled in the ridge pattern diagram
Answer: The suspected and crime scene fingerprint patterns are similar which means they belong to the same individual.
Explanation:
A: Ending ridge between two lines forming a loop like structure common in both suspected and crimes scene patterns.
B: Bifurcation which includes the formation of fork like shape of the ridge.
C: Island is a dot or point like structure which is common in both patterns.
D: It includes delta which is seen in the case of loop and whorl patterns of the fingerprint in loop there is only one delta and in case of whorl there are two deltas. The delta have an island and a bifurcation in it which is common in both patterns of the fingerprints.
E: Intersection occurs when two ridges changes their directions. It is common in the two patterns.
Calculate the molarity of a MgSosolution
prepared by adding 0.37 moles of MgSO, to
enough water to make 11 of solution.
Answer in units of V.
Answer:
is
Explanation:
because
If you obtain 3.0 grams of aspirin from an experiment that could make no more than 3.14 grams, what is the percent yield?
87%
105%
96%
92%
Answer:
96%
Explanation:
To find the percent yield, we can use this equation
[tex]\frac{Actual}{Theoretical} *100[/tex]
The actual yield of aspirin is 3.0 and the theoretical is 3.14 in this case, so just plug the numbers in.
[tex]\frac{3.0}{3.14} *100\\\\ =96[/tex]
Thus the percent yield is 96%
;)
dentify whether each element is a halogen, a noble gas, or nonmetal only.
Astatine (At):
Nitrogen (N):
Krypton (Kr):
Chlorine (Cl):
Sulfur (S):
Astatine : Halogen
Nitrogen : Nonmetal
Krypton : Noble gas
Chlorine : Halogen
Sulfur : Nonmetal
i just needed the points sorryyy
A solution is made from 0.5 moles of sodium dichromate. If the volume of the solution is 1 Liter, what is the molarity of the solution
2 M
0.5 M
4 M
1 M
Answer:
4 M
Explanation:
See the steps and explanation in the picture
Which refers to the force that one massive object exerts to attract another object?
velocity
gravity
acceleration
newt
Answer:
acceleration
mhmm..whichuksnackru?..fishnchiips OUHHHOOUUHHYESS SandyROASTthatsevenbaetterthanfishnchips
Which equation represents neutralization?
(1 ) 6Li(s)+N 2 (g)=>2Li3N(s)(2) 2Mg(s)+O2(g)=>2MgO(s) (3) 2KOH(aq)+H2SO4(aq) =>K 2 SO 4 (aq)+2H 2 O(l)
(4) Pb(NO 3 ) 2 (aq)+K 2 CrO 4 (aq) => 2KNO 3 (aq)+PbCrO 4 (s)
Answer:
3) 2KOH(aq) + H2SO4(aq) ⇒ K2SO4(aq) + 2H2O(l)
Explanation:
KOH is a strong base and a H2SO4 is a strong acid. The two react in a neutralization reaction, producing a salt and water.
Which material would conduct heat best?
А.Air
B.Copper
C.Wood
D.Rubber
Answer:
I believe the best answer is B. Copper.
Combustion Analysis of an unknown hydrocarbon resulted in the capture of 216.00 g of water vapor and 440.00 g of CO2. The total mass of the hydrocarbon before combustion was 144 g.
(1. How many moles of carbon dioxide are present after combustion?)
(2. What is the empirical formula for the unknown hydrocarbon?)
(3. How many water molecules does the water vapor trap capture?)
(4. The gram-formula mass for the unknown hydrocarbon was determined to be 72 g/mol. How many moles of the unknown hydrocarbon were present in the original sample?)
(5. infrared spectral analysis determines that the unknown hydrocarbon does NOT contain oxygen. How many moles of O2 are used in combusting the unknown sample?)
1: 10 mol CO2
2: C10H24
3: 12 mol H2O
4: 0.5 mol
5: 16 mol O2
The compound is C5H10.
From the information available in the question;
Number of moles of carbon dioxide = 440.00 g/44 g/mol = 10 moles
Number of moles of water vapor = 216.00 g/18 g/mol = 12 moles
Mass of carbon = 10 moles × 12 g/mol = 120 g of carbon
Moles of hydrogen = 12 moles × 2 g/mol = 24 g of hydrogen
Number of moles of carbon = 120 g/12 g/mol = 10 moles
Number of moles of hydrogen = 24 g/1 g/mol =24 moles
Divide through by the lowest number of moles =
C - 10/10 H - 24/10
C - 1 H - 2
The empirical formula is CH2
Molar mass of the compound = 72 g/mol
[12 + 2(1)]n = 72
14n = 72
n = 5
The compound is C5H10.
Learn more about hydrocarbons: https://brainly.com/question/1195122
consider the following atoms and ion: Cl,Mg,P,K,Ce =
A)which one is an example of ns² family?
B)which one is an example of p-block element?
C) which is (are) isoelectronic with Argon?
D) Which one is an example of alkaline earth metal?
E) which one has core configuration [Ne]3s²?
F) which one is an example of f-block element?
G) which one is d-block element?
H) which one has outer shell configuration of ns²p³?
Answer:it would be f
Explanation:
What is the concentration of kl solution if 20.68g of solute was added to enough water to form 100ml solution?
Answer:
1.25 M
Explanation:
Step 1: Given data
Mass of KI (solute): 20.68 g
Volume of the solution: 100 mL (0.100 L)
Step 2: Calculate the moles of solute
The molar mass of KI is 166.00 g/mol.
20.68 g × 1 mol/166.00 g = 0.1246 mol
Step 3: Calculate the molar concentration of KI
Molarity is equal to the moles of solute divided by the liters of solution.
M = 0.1246 mol/0.100 L= 1.25 M
does anyone know the answer???
Answer:
ethyl ethernal
Explanation:
no explanation
Which of the following is true according the the Arrhenius theory of acids?
A strong acid increases the OH-ion concentration in an aqueous solution.
A strong acid decreases the OH-ion concentration in an aqueous solution.
O A strong acid decreases the H+ and OH-ion concentration in an aqueous
solution.
A strong acid increases the H+ ion concentration in an aqueous solution.
A compound has the empirical formula CH20 and a
gram-formula mass of 60. grams per mole. What is the
molecular formula of this compound?
Answer:
The molecular formula of this compound is (2) C2H4O2.
Explanation:
Combustion of hydrocarbons such as octane (C_8H_18) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide.
1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid octane into gaseous carbon dioxide and gaseous water.
2. Suppose 0.330 kg of octane are burned in air at a pressure of exactly 1 atm and a temperature of 10.0 ?C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits.
Answer: 1. [tex]2C_8H_{18}(l)+25O_2(g)\rightarrow 16CO_2(g)+18H_2O(g)[/tex]
2. The volume of carbon dioxide gas that is produced is 537 L
Explanation:
1. Combustion is defined as the type of chemical reaction where a hydrocarbon is combusted in the presence of oxygen to give carbon dioxide and water.
The balanced reaction for combustion of octane is:
[tex]2C_8H_{18}(l)+25O_2(g)\rightarrow 16CO_2(g)+18H_2O(g)[/tex]
2.
To calculate the moles :
[tex]\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}[/tex] [tex]\text{Moles of octane}=\frac{0.330\times 1000g}{114.23g/mol}=2.89moles[/tex]
According to stoichiometry:
2 moles of octane produce = 16 moles of carbon dioxide
2.89 moles of octane produce = [tex]\frac{16}{2}\times 2.89=23.1moles[/tex] of carbon dioxide
According to ideal gas equation:
[tex]PV=nRT[/tex]
P = pressure of gas = 1 atm
V = Volume of gas = ?
n = number of moles = 23.1
R = gas constant =[tex]0.0821Latm/Kmol[/tex]
T =temperature =[tex]10.0^0C=(10+273)K=283K[/tex]
[tex]V=\frac{nRT}{P}[/tex]
[tex]V=\frac{23.1\times 0.0821Latm/K mol\times 283K}{1atm}=537L[/tex]
Thus the volume of carbon dioxide gas that is produced is 537 L
Balance the following equations:
C3H8 (g) + O2 (g) → CO2 (g) + H2O (g)
NH3 (g) O2 (g) NO2 (g) H2O (g)
Al(NO3) Na3S Al2S3 NaNO3
Explanation:
C3H8 + 502 ----> 3CO2 + 4H20
4NH3+7O2------> 4NO2+6H2O
2Al(NO3)3 + 3Na2S -------> Al2S3+6NaNO3
Explain why water and syrup are able to mix?
How many molecules of CO2 at standard temperature and pressure in 5.4 moles of CO2
Answer:
3.25×10²⁴ molecules.
Explanation:
From the question given above, the following data were obtained:
Number of mole of CO₂ = 5.4 moles
Number of molecules of CO₂ =?
The number of molecules of CO₂ in 5.4 moles can be obtained as follow:
From Avogadro's hypothesis,
1 mole of CO₂ = 6.02×10²³ molecules
Therefore,
5.4 moles of CO₂ = 5.4 × 6.02×10²³
5.4 moles of CO₂ = 3.25×10²⁴ molecules
Thus, 5.4 moles of CO₂ contains 3.25×10²⁴ molecules.
PLEASE HELP WILL GIVG BRAINLEST
Answer:
It is option #1.
Explanation:
Biotechnology is defined as, "The exploitation of biological processes for industrial and other purposes, especially the genetic manipulation of microorganisms for the production of antibiotics, hormones, etc."
Therefore, option #1 is your answer!
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Calculate AEfor a system that absorbs 599,0 kJ of heat from its surroundings
and does 3510 kJ of work on its surroundings.
Answer:
-2911 kJ
Explanation:
Step 1: Given data
Heat absorbed by the system (Q): 599.0 kJ (By convention, when the systems absorbs heat, Q > 0)Work done by the system on the surroundings (W): -3510 kJ (By convention, when the systems does work on the surroundings, W < 0)Step 2: Calculate the change in the internal energy (ΔE)
We will use the following expression.
ΔE = Q + W
ΔE = 599.0 kJ + (-3510 kJ) = -2911 kJ