For the reaction, $2 A + B \to A_{2} B$ the rate $= k [A] [B]^{2}$ with $k = 2.0 \times 10^{- 6} m o l^{- 2} L^{- 2} s^{- 1}$ . Calculate the initial rate of reaction when $[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1}$ . Calculate the rate of reaction after [A] is reduced to $0.06 m o l L^{- 1}$ .

Q. For the reaction:

2 A + B \to A_{2} B

, the rate

= k [A] [B]^{2}

with

k = 2.0 \times 10^{- 6} m o l^{- 2} L^{2} s^{- 1}

Calculate the initial rate of the reaction when

[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1}

. Calculate the rate of reaction after

[A]

is reduced to

0.06 m o l L^{- 1}

Join BYJU'S Learning Program

The rate of the reaction, 2NO+O2⟶2NO2, at 25oC is 0.028 mol L−1s−1. The experimental rate is given by, r=k[NO]2[O2].If the initial concentrations of the reactants are O2=0.040 mol L−1 and NO=0.01 mol L−1, the rate constant of the reaction is:

The correct option is D 7.0×103 L2 mol−2s−1r=k[NO]2[O2] Now, using given quantities:0.028=k.(0.04)(0.01)k=7×10−3L2mol−2s−1

The correct option is D $7.0 \times 10^{3} L^{2} {m o l}^{- 2} s^{- 1}$
$r = k [N O]^{2} [O_{2}]$
Now, using given quantities:
$0.028 = k . (0.04) (0.01) k = 7 \times 10^{- 3} L^{2} {m o l}^{- 2} s^{- 1}$