Final answer:
The heat consumed when 5.10 g of CO (g) is formed is +23.43 kJ.
Step-by-step explanation:
To find the amount of heat consumed when 5.10 g of CO (g) is formed, we need to use the given ΔH° value and the stoichiometry of the reaction. The balanced equation is:
CH₃OH (l) → CO (g) + 2H₂ (g)
From the equation, we can see that 1 mole of CO (g) is produced from 1 mole of CH₃OH (l). We can use molar mass to convert the mass of CO (g) to moles:
Mr of CO (g) = 28.01 g/mol
moles of CO (g) = mass of CO (g) / molar mass
moles of CO (g) = 5.10 g / 28.01 g/mol = 0.1828 mol
Finally, we can use the ΔH° value to calculate the heat consumed:
Heat consumed = moles of CO (g) * ΔH°
Heat consumed = 0.1828 mol * +128.1 kJ/mol = +23.43 kJ