Final answer:
To give off 1501 kJ of heat in the given reaction, 2.34 moles of CH3OH are required. Solving for x, we find that x = (1501 kJ) / (640 kJ/mol) = 2.34 mol of CH₃OH.
Step-by-step explanation:
To determine how many moles of CH3OH are required to give off 1501 kJ of heat in the given reaction: 2 CH₃OH (l) + 3 O₂ (g) → 2 CO₂ (g) + 4 H₂O(g) with a ΔH° = -1280 kJ/mol, we can use the concept of stoichiometry and the given enthalpy change.
The balanced equation shows that 2 moles of CH₃OH are required to produce 2 moles of CO₂ and 4 moles of H₂O.
From the reaction, we can see that the enthalpy change of -1280 kJ/mol corresponds to the formation of 2 moles of CO₂ and 4 moles of H₂O.
Therefore, for the formation of 1 mole of CO₂, the enthalpy change is -1280 kJ/2 = -640 kJ/mol.
So, to determine the moles of CH₃OH required for 1501 kJ of heat, we can set up the following proportion: (-1280 kJ/mol) / 2 mol of CO₂ = (-640 kJ/mol) / x mol of CH₃OH.
Solving for x, we find that x = (1501 kJ) / (640 kJ/mol) = 2.34 mol of CH₃OH.