Question: Consider a reaction A(g)¾® 3 B(g) + 2C(g) with rate constant 1.386 ...

Question

Consider a reaction A_(g)¾® 3 B_(g) + 2C_(g) with rate constant 1.386 × 10^–2 min^–1. Starting with 2 moles of A in 12.5 litre vessel, if reaction is allowed to takes place at constant pressure & at 298 K then find the concentration of B after 100 min -

Answer 1

Solution

K = $\frac{0.693}{t_{1/2}}$ or t_1/2 = $\frac{0.693}{1.38 \times 10^{–2}}$ = 50 min

A_(g) ¾® 3B_(g) + 2C_(g)

after 2 – x 3x 2x

100 min = 0.5 4.5 3

$\frac{V_{f}}{V_{i}}$ = $\frac{n_{f}}{n_{i}}$ Ž V_f = $\frac{8}{2}$ × 12.5 Ž 50 Lit

\ Concentration of B after

100 min = $\frac{4.5}{50}$ = 0.09 M

Question: Consider a reaction A<sub>(g)</sub>¾® 3 B<sub>(g)</sub> + 2C<sub>(g)</sub> with rate constant 1.386 ...

Solution