The value of ΔH° for the reaction below is +128.1 kJ: CH₃OH (l) → CO (g) + 2H₂ (g)
How many kJ of heat are consumed when 5.10 g of CO (g) is formed as shown in the equation?

Question

Quizplus · Accepted Answer

First, we need to calculate the moles of CO produced:

n(CO) = m/M = 5.10g/28.01 g/mol = 0.1827 mol

Then, we can use the stoichiometry of the reaction to calculate the moles of CH3OH consumed:

1 mol CH3OH produces 1 mol CO

Δn(CH3OH) = -n(CO) = -0.1827 mol

Finally, we can use the equation:

ΔH° = q/n

where q is the heat absorbed or released and n is the number of moles of reactant or product in the reaction.

q = ΔH° × n = 128.1 kJ/mol × 0.1827 mol = 23.34 kJ

Therefore, the answer is D) 23.3 kJ.

The Value of ΔH° for the Reaction Below Is +128