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?

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):

[tex]152g*\frac{1mol}{30.01g} =5.065mol[/tex]

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

[tex]5.065mol*\frac{43kcal}{2mol} =108.9kcal[/tex]

Which kJ turns out:

[tex]108.9kcal*\frac{4.184kJ}{1kcal}\\\\455.6kJ[/tex]

Best regards!

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?

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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?