Log in
HomeClass Notes1,200,000CA670,000

CHY 103 Lecture Notes - Lecture 6: Joule, Ammonium Nitrate, Heat Capacity

17 views8 pages
School
Ryerson University
Department
Chemistry
Course
CHY 103
Professor
Noel George

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

If we consider that h final in our system represents the products and h initial corresponds to the reactants then we can write the following: Since the above equation represents the enthalpy change for a chemical reaction we sometimes signify it by rh and include it with the balanced equation. 2h2(g) + o2(g) 2 h2o (g) rh = - 483. 6 kj mol-1. The enthalpy change for a reaction can be represented by an _____________________. Enthalpy is an _____________, meaning that the magnitude of rh is directly proportional to the amount of reactant consumed in the process. The enthalpy change for a reaction is equal in magnitude _____________ in sign to rh for the reverse reaction. The enthalpy change for a reaction depends on the state of the reactants and products. 2 n2(g) + o2(g) 2 n2o(g) rh = 163. 2 kj mol-1 (a) is the reaction exothermic or endothermic? (b) calculate the amount of heat transferred when.

Get access

Grade+
$40 USD/m
Billed monthly
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
10 Verified Answers
Class+
$30 USD/m
Billed monthly
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
7 Verified Answers

Related Documents

CHY 103 Lecture Notes - Lecture 9: Bond-Dissociation Energy, Joule, Calcium Carbide
plumgoat724
CHY 103 Lecture Notes - Lecture 6: Calcium Carbide, Joule
amaranthjackal682
CHY 103 Lecture Notes - Lecture 2: Reagent, Chemical Equation
goldchinchilla75

Related Questions

We need help on a Gen Chem 1 Calorimetry and Enthalpy lab and the TA for the class wasn't much help at all.

1) Did the reaction absorb or release heat. Using the value of q you calculated, calculate del H of the reaction in kJ/mol of reactant. (start by calculation q for the reaction; don't forget the role of the calorimeter.) (our answer is -1.8kJ, but we know this must be incorrect since the TA got approx -51 kJ and then wouldn't show us what we did wrong.)

2)Write a balanced thermochemical equation for this reaction, including the value of del H

Reactant 1 (NaOH)
mass: 52.00g
volume: 50.0mL.
moles: 1.3 mol

Reactant 2 (HCl; density=1.017g/mL)
mass: 50.85g
volume: 50.00mL
moles: 1.4 mol

Solution:
mass: 102.85g
volume: 100 mL
Tinitial: 24.1C
Tfinal: 29.0C
delT: 4.9C
c for Sol: 3.97 J/g*C
q= 2000J (calculated using q=mc(del)T


1- The molar heat capacity of silver is 25.35 J/mol⋠∘C. How much energy would it take to raise the temperature of 8.20 g of silver by 14.5 ∘C?

Express your answer with the appropriate units.

_____________

Part A

Calculate the enthalpy of the reaction

2NO(g)+O2(g)→2NO2(g)

given the following reactions and enthalpies of formation:

12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ

12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ

Express your answer with the appropriate units.

2- A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 196 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 ∘C. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water.

Enter your answer in kilojoules per mole of compound to three significant figures.

_________

3- A volume of 110. mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘Cis placed in the water. If the final temperature of the system is 21.00 ∘C , what is the mass of the steel bar?

Use the following values:

specific heat of water = 4.18 J/(g⋠∘C)

specific heat of steel = 0.452 J/(g⋠∘C)

Express your answer to three significant figures and include the appropriate units.

Part B

The specific heat of water is 4.18 J/(g⋠∘C). Calculate the molar heat capacity of water.

Express your answer to three significant figures and include the appropriate units.

______-

4- What is the enthalpy for the following reaction?

overall: N2O4→2NO2

Express your answer numerically in kilojoules per mole.

____________

Part B

Calculate the enthalpy of the reaction

4B(s)+3O2(g)→2B2O3(s)

given the following pertinent information:

B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ

2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ

H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ

H2O(l)→H2O(g), ΔH∘D=+44 kJ

Express your answer with the appropriate units.

_____________

5- What is the balanced chemical equation for the reaction used to calculate ΔH∘f of MgCO3(s)?

If fractional coefficients are required, enter them as a fraction (i.e. 1/3). Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution.

Express your answer as a chemical equation.

__________

6- Part A

Determine the enthalpy for this reaction:

Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l)

Express your answer in kilojoules per mole to one decimal place.

_______

Part B

Consider the reaction

Ca(OH)2(s)→CaO(s)+H2O(l)

with enthalpy of reaction

ΔHrxn∘=65.2kJ/mol

What is the enthalpy of formation of CaO(s)?

Express your answer in kilojoules per mole to one decimal place.

________

7- Part A

Write a balanced chemical equation depicting the formation of one mole of H2O2(g) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

_____

Part B

For H2O2(g), find the value of ΔH∘f. (Use Appendix C)

Express your answer using five significant figures.

_____

PART C: Write a balanced chemical equation depicting the formation of one mole of CaCO3(s) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

_____

Part D

For CaCO3(s), find the value of ΔH∘f. (Use Appendix C)

Express your answer using five significant figures.

_____

Part E

Write a balanced chemical equation depicting the formation of one mole of POCl3(l) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

____

Part F

For POCl3(l), find the value of ΔH∘f. (Use Appendix C)

Express your answer using four significant figures.

_____

Part G

Write a balanced chemical equation depicting the formation of one mole of C2H5OH(l) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

_____

Part H

For C2H5OH(l), find the value of ΔH∘f. (Use Appendix C)

Express your answer using four significant figures.