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11 Dec 2019

Calculate the ΔH∘ for this reaction using the following thermochemical data:

CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ
C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ
2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ
2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l) ΔH∘=−3120.8kJ

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

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Related questions

Top fuel dragsters and funny cars burn nitromethane as fuel according to the following balanced combustion equation:
2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(g)+N2(g)
The standard enthalpy of combustion for nitromethane is −709.2kJ/mol.

Calculate the standard enthalpy of formation (ΔH∘f) for nitromethane.

Express your answer using four significant figures.

PART A:Click the DeltaH is an Extensive Property button within the activity, and analyze the relationship between the two reactions that are displayed. The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, ΔH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2. Reaction 1: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g), ΔH1=−2043 kJ Reaction 2: 4C3H8(g)+20O2(g)→12CO2(g)+16H2O(g), ΔH2=? Express your answer to four significant figures and include the appropriate units.

PART B: analyze the relationship between the two reactions that are displayed. The reaction that was on the screen when you started and its derivative demonstrate that the reaction enthalpy, ΔH, changes sign when a process is reversed. Consider the reaction B(s)+32O2(g)→B2O3(s), ΔH =−1270kJ

PART C:What will ΔH be for the reaction if it is reversed? alculate the reaction enthalpy, ΔH, for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(l)Use the series of reactions that follow: C(s)+2H2(g)→CH4(g), ΔH =−74.8 kJ. C(s)+O2(g)→CO2(g), ΔH =−393.5 kJ. 2H2(g)+O2(g)→2H2O(g), ΔH =−484.0 kJ. H2O(l)→H2O(g), ΔH =44.0 kJ. Express your answer with appropriate units.

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.

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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.

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