Question

One mole (mol) of nitrogen monoxide (NO) has a mass of 30.01 g. When

precisely 2 moles of NO(g) are produced in the following chemical reaction, 43
kcal of heat energy is "absorbed."
N2(g) + O2(g) → 2 NO(g), AH = +43 kcal
How much heat (in kJ) is exchanged when 152 g of NO(g) is produced?

Answer 1

455.6 kJ.

Step-by-step explanation:

Hello there!

In this case, according to the given reaction, we know that 2 moles of NO require 43 kcal of energy, thus, for the energy required by 150 g of NO we first need the moles, considering its molar mass (30.01 g/mol):

`152g*(1mol)/(30.01g) =5.065mol`

Thus, we apply the following dimensional analysis to obtain the energy absorbed by 5.065 moles:

`5.065mol*(43kcal)/(2mol) =108.9kcal`

Which kJ turns out:

`108.9kcal*(4.184kJ)/(1kcal)\\\\455.6kJ`

Best regards!