What is the standard enthalpy of reaction for the following chemical reaction?

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

Express your answers numerically in kJ.

-148.9

Well, I could tell you the standard enthalpy of reaction for that chemical reaction, but it's classified information. If I told you, I'd have to dissolve you in a vat of hydrochloric acid. And no one wants that, right?

To determine the standard enthalpy of reaction for the given chemical equation, you need to know the standard enthalpies of formation for each of the compounds involved. The standard enthalpy of formation (ΔHf°) is the heat change when one mole of a compound is formed from its elements in their standard states at a given temperature and pressure.

First, we need to gather the values of the standard enthalpies of formation for each compound involved in the reaction. The standard enthalpies of formation can be found in reference tables or chemical databases. For this question, the standard enthalpies of formation at 25°C and 1 atm are as follows:

ΔHf° (CO2) = -393.5 kJ/mol
ΔHf° (KOH) = -424.0 kJ/mol
ΔHf° (H2O) = -241.8 kJ/mol
ΔHf° (K2CO3) = -1150.6 kJ/mol

Now, we can calculate the standard enthalpy of reaction using the formula:

ΔH° = Σ(nΔHf° products) - Σ(nΔHf° reactants)

In this equation, n represents the stoichiometric coefficients of each compound in the balanced chemical equation.

Let's calculate it step by step:

Reactants:
1 CO2(g): nΔHf° = 1 * (-393.5 kJ/mol)
2 KOH(s): nΔHf° = 2 * (-424.0 kJ/mol)

Products:
1 H2O(g): nΔHf° = 1 * (-241.8 kJ/mol)
1 K2CO3(s): nΔHf° = 1 * (-1150.6 kJ/mol)

Now, substitute the values into the formula:

ΔH° = [1*(-241.8 kJ/mol) + 1*(-1150.6 kJ/mol)] - [1*(-393.5 kJ/mol) + 2*(-424.0 kJ/mol)]

Simplify the equation:

ΔH° = (-241.8 kJ/mol - 1150.6 kJ/mol) - (-393.5 kJ/mol - 2*(-424.0 kJ/mol))
ΔH° = -1392.4 kJ/mol + 430.5 kJ/mol

Finally, calculate the value:

ΔH° = -961.9 kJ/mol

Therefore, the standard enthalpy of reaction for the given chemical equation is -961.9 kJ/mol.

You need to look these values up, individually, in a set of tables. Then

delta H rxn = delta H products - delta H reactants.

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