The value of ΔH° for the reaction below is +128.1 kJ: CH₃OH (l)→ CO (g)+ 2H₂ (g) How much heat is consumed when 87.1 g of hydrogen gas is formed? A)2.76 × 10³ kJ B)5.52 × 10³ kJ C)-5.52 × 10³ kJ D)-2.76 × 10³ kJ E)-128.1 kJ

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Quizplus · Accepted Answer

The reaction produces 2 moles of hydrogen gas for every mole of CH3OH consumed, with a ΔH° of +128.1 kJ. The molar mass of H2 is approximately 2.02 g/mol, so 87.1 g of H2 corresponds to 87.1 g / 2.02 g/mol ≈ 43.1 moles of H2. Since the given ΔH° is for the production of 2 moles of H2, the heat consumed for 43.1 moles is (43.1 moles / 2 moles) * 128.1 kJ = 2765.55 kJ, which is approximately 2.76 × 10^3 kJ.

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