For 2(g) + (g) - 2(g); δ H = -35.0 kcal at 300 K. If 6.0 moles of reacts with 3.0 moles of at constant pressure at 300 K, the correct statement(s) is/are

Question

For 2$NO_2$(g) + $O_2$(g) -> 2$NO$(g); δ H = -35.0 kcal at 300 K. If 6.0 moles of $NO$ reacts with 3.0 moles of $O_2$ at constant pressure at 300 K, the correct statement(s) is/are

Prashant Kotian · Accepted Answer

Correct answer: A,D. Reverse: 2(g) + (g) -> 2(g); δ H = -35 kcal for 2 mol . For 6 + 3 -> 6: δ H = 3*(-35) = -105 kcal. δ n_g = 6 - 9 = -3. W = δ n_g * RT = -3 * 2 * 300 cal = -1800 cal = -1.8 kcal (magnitude 1.8 kcal, A correct). Book key uses δ E = δ H +

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