Part A What is H rxn for the following chemical reaction? CO2(g)+2KOH(s)H2O(g)+K

Question

Part A

What is Hrxn for the following chemical reaction?

CO2(g)+2KOH(s)H2O(g)+K2CO3(s)

You can use the following table of standard heats of formation (Hf) to calculate the enthalpy of the given reaction.

Express the standard enthalpy of reaction to three significant figures and include the appropriate units.

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Part B

What volume of methanol is formed if 2.92×1011 L of methane at standard atmospheric pressure and 25 C is oxidized to methanol? The density of CH3OH is 0.791 g/mL. Assume that the oxidation of methane to methanol occurs in a 1:1 stoichiometry.

Express your answer numerically in liters.

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Standard heats of formation

The standard heats of formation for selected substances are shown here.

Part C

Calculate the standard enthalpy changes for the combustion of a mole of methane and the combustion of a mole of methanol.

Enter the enthalpy for methane followed by the enthalpy for methanol in kilojoules separated by a comma using four significant figures.

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Part D

Consider the reaction

Ca(OH)2(s)CaO(s)+H2O(l)

with enthalpy of reaction

Hrxn=65.2kJ/mol

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

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

Hints

N2H4(l)+N2O4(g)2N2O(g)+2H2O(g)

Standard Enthalpies of Formation at 25 C

Part E

Calculate Hrxn for this reaction using standard enthalpies of formation.

Express your answer using one decimal place.

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Ethanol can be made from the fermentation of crops and is used as a fuel additive to gasoline.

Part F

Write a balanced equation for the combustion of ethanol (assume the water as a product of reaction to be gaseous).

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

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Part G

Calculate Hrxn.

Express your answer using four significant figures.

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Element/ Compound Standard Heat of Formation (kJ/mol) Element/ Compound Standard Heat of Formation (kJ/mol) H(g) 218 N(g) 473 H2(g) 0 O2(g) 0 KOH(s) 424.7 O(g) 249 CO2(g) 393.5 K2CO3(s) 1150kJ C(g) 71 H2O(g) 241.8kJ C(s) 0 HNO3(aq) 206.6

Explanation / Answer

Question 1.

HRXN = CO2(g)+2KOH(s)H2O(g)+K2CO3(s)

For the heat of reaction, we need the change of each species

From th eheat of reaction:

HRXN = Hproducts - Hreactants

where Hprod = enthalpy of formation of products

and Hreact = enthalpy of formation of reactants

then, substitute values from the equation given:

HRxn = H2O + K2CO3 - (CO2 + 2*KOH)

HRxn= -241.8 + -1150 - (-393.5 + 2*-424.7)

HRxn = -148.9 kJ

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