Question

For a reaction A + B → C + 2D, experimental results were
collected for three trials and the data obtained are given
below:
Trial [A], M [B], M Initial Rate, M s⁻¹
1 0.40 0.20 5.5 × 10⁻⁴
2 0.80 0.20 5.5 × 10⁻⁴
3 0.40 0.40 2.2 × 10⁻³
The correct rate law of the reaction is
(a) rate = k[A]⁰ [B]² (b) rate = k[A] [B]²
(c) rate = k[A] [B] (d) rate = k[A] [B]⁰

Answer 1

c is correct

Explanation:

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Answer 2

rate law of the reaction is k[A]⁰ [B]²

• [A] M [B] Initial Rate

1 0.40 0.20 5.5 × 10⁻⁴

2 0.80 0.20 5.5 × 10⁻⁴

3 0.40 0.40 2.2 × 10⁻³

• let Rate = k[A]^m[B]^n

• keeping [B] = const.

• Rate is proprtional to [A]^m

• On Doubling A rate remains same

( From (1) & (2) )

• [A] has no effect on rate

• m =0

• keeping [A] = const.

• Rate is proprtional to [B]^m

• On Doubling B rate increases by

4 times from (1) & (2)

•This means, Rate according to B is

second order

order

• n =2

• rate = k[A]⁰ [B]²