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 15.5 g of CH₃OH (l) decomposes 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 15.5 g of CH₃OH (l)decomposes as shown in the equation?

Quizplus · Accepted Answer

First, we need to calculate the moles of CH₃OH used in the reaction: 15.5 g CH₃OH x (1 mol / 32.04 g) = 0.483 mol CH₃OH Next, we use the stoichiometry of the reaction to calculate the amount of heat consumed: 0.483 mol CH₃OH x (+128.1 kJ / 1 mol CH₃OH) = +62.0 kJ Since the value of ΔH° is positive, energy is absorbed from the surroundings, which means heat is consumed. Therefore, the answer is B.

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