ThermochemistryHard

Question

For the reaction, 2NO(g) + O2(g) → 2NO2(g); ΔH = −35.0 kcal at 300 K. If 6.0 moles of NO reacts with 3.0 moles of O2 at constant pressure of 1.0 atm and temperature 300 K to form NO2, then which of the following statement(s) is/are correct?

Options

A.The magnitude of work done by the system is 1.8 kcal.
B.The amount of heat released by the reaction is 35 kcal.
C.The internal energy of system decreased by 103.2 kcal.
D.The internal energy of system decreased by 106.8 kcal.

Solution

$\Delta H = q = 3 \times ( - 35) = - 105\text{ kcal}$

$\Delta U = \Delta H - \Delta n_{g}RT $$${ = \left\lbrack ( - 35) - (2 - 3) \times \frac{2}{1000} \times 300 \right\rbrack \times 3 = - 103.2\text{ kcal} }{\text{and }w = u - q = ( - 103.2) - (105) = 1.8\text{ kcal}}$$

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