Question

According to the equation $C_6{H}_{6\left(l\right)}+\frac{15}{2}{O}_{2\left(g\right)}\to 3H_2{O}_{\left(i\right)}+6C{O}_{2\left(g\right)}$ $\Delta H=-3264.4kJ/mol$, the energy evolved when 7.8 g of benzene is burnt in air will be :

• A. 163.22 kJ/mol
• B. 326.4 kJ/mol
• C. 32.64 kJ/mol
• D. 3.264 kJ/mol

Answer 1

The correct option is B 326.4 kJ/mol

Device $1$ mole of benzene requires -$3264.4K5$

$\left(\frac{7.8}{78}\right)$ mole of benzene requires $\left(\frac{-3264.4\times 0.1}{1}\right)K5$

$\equiv -326.44K5/mole.$