CH₃OH (l)decomposes into carbon monoxide and hydrogen gas in the presence of heat.How much heat is consumed when 5.75 g of CO (g)is formed? ΔH° = +128.1 kJ.

Question

Quizplus · Accepted Answer

The balanced chemical equation for the decomposition of CH₃OH (l) is: CH₃OH (l) → CO (g) + H2 (g) We are given that ΔH° = +128.1 kJ for this reaction. This means that 128.1 kJ of heat is absorbed for the formation of 1 mole of CO (g) from CH₃OH (l). To find the amount of heat consumed for the formation of 5.75 g of CO (g), we need to first calculate the number of moles of CO (g) formed: 1 mole of CO (g) is formed from 1 mole of CH₃OH (l). The molar mass of CO is 28.01 g/mol. Therefore, 5.75 g of CO is: 5.75 g ÷ 28.01 g/mol = 0.205 mole of CO (g) From the balanced equation, we see that 1 mole of CO (g) is formed with consumption of ΔH° = +128.1 kJ. Therefore, 0.205 mole of CO (g) will form with a consumption of: ΔH = 0.205 mole × (+128.1 kJ/mole) = 26.3 kJ Hence, the answer is A)26.3 kJ.

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