Question

When 1 mol of methane is burned at constant pressure, −890 kJ/mol of energy is released as heat. If a 1.67 g sample of methane is burned at constant pressure, what will be the value of ∆H

Answer 1

Answer:

$\Delta H=-92.7kJ$

Explanation:

Hello there!

In this case, according to the given information, we can infer that 890 kJ of energy are released when 1 mole of methane is burned; however, to find the total heat when 1.67 grams are burned, we first need to calculate the moles in this mass of methane:

$1.67gCH_4*\frac{1molCH_4}{16.04gCH_4}=0.104molCH_4$

And thus, for calculating the resulting ∆H, we proceed as follows:

$\Delta H=-890kJ/mol*0.104mol\\\\\Delta H=-92.7kJ$

Regards!