Consider the following equation: CO + 2 H₂ → CH₃OH △H rxn = -128 kJ Calculate the amount of heat (in kJ)associated with complete reaction of 8.08 g H₂.

Question

Quizplus · Accepted Answer

First, we need to balance the chemical equation. After balancing, we have:

CO + 2 H2S -> CH2S + H2O

From the equation, we know that the enthalpy change for the reaction is -128 kJ. This means that for every 128 kJ of heat released, one mole of CO and 2 moles of H2S react to form one mole of CH2S and one mole of H2O.

To calculate the amount of heat released by reacting 8.08 g of H2S, we need to first convert the mass of H2S to moles. The molar mass of H2S is 34.08 g/mol, so:

8.08 g H2S x (1 mol H2S/34.08 g H2S) = 0.237 mol H2S

Because 2 moles of H2S react for every mole of CH2S produced, we know that 0.1185 moles of CH2S will be produced. Using the enthalpy change from the balanced equation, we can calculate the amount of heat released as:

128 kJ/1 mole x 0.1185 moles = 15.16 kJ

Therefore, the amount of heat released by reacting 8.08 g of H2S is -15.16 kJ, or approximately -256 kJ. The answer is (C).

Consider the Following Equation: CO + 2 H2 → CH3OH

Consider the Following Equation: CO + 2 H₂ → CH₃OH