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

Question

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

Quizplus · Accepted Answer

Using the given ΔH°, we can calculate the amount of heat consumed for the formation of 1 mole of CO as follows:
ΔH° = +128.1 kJ/mol
We want to find the heat consumed for the formation of 5.10 g of CO, which is:
moles of CO = mass/molar mass = 5.10 g/28.01 g/mol = 0.1827 mol CO
Heat consumed = moles of CO × ΔH° = 0.1827 mol CO × 128.1 kJ/mol = 23.32 kJ (rounded to two decimal places)

Therefore, the correct answer is D.

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