Question

The value of $\Delta H-\Delta E$ for the following reaction at ${27}^o$C will be, $2N{H}_3\left(g\right)\to N_2\left(g\right)+3H_2\left(g\right)$:

• A. $8.314\times 273\times (-2)J$
• B. $8.314\times 300\times (-2)J$
• C. $8.314\times 27(+2)J$
• D. $8.314\times 300(+2)J$

Answer 1

Answer: (D)

$8.314\times 300(+2)J$

$△n=4-2=2$

$R=8.314$

$T=27C=300K$

$△H=△E+△nRT$

$\Rightarrow △H-△E=△nRT$

$=2\times 8.314\times 300$