Compounds 'A' and 'B' react according to the following chemical equati

1.	Compounds 'A' and 'B' react according to the following chemical equation. A(g)+2B(g)⟶2C(g) Concentration of either 'A' or 'B' were changed keeping the concentration of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction. ExperimentInitial Concentration of [A]/moIL−1Initial cooncentration of [B]/moIL−1Initial cooncentration of [C]/moIL−1s−11.0.300.300.102.0.300.600.403.0.600.300.20 (a)Rate=k[A]2[B] (b)Rate=k[A][B]2(c)Rate=k[A][B] (d)Rate=k[A]2[B]0
Answer» Compounds 'A' and 'B' react according to the following chemical equation. $A (g) + 2 B (g) ⟶ 2 C (g)$ Concentration of either 'A' or 'B' were changed keeping the concentration of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction. $\begin{matrix} E x p e r i m e n t & I n i t i a l C o n c e n t r a t i o n o f [A] / m o I L^{- 1} & I n i t i a l c o o n c e n t r a t i o n o f [B] / m o I L^{- 1} & I n i t i a l c o o n c e n t r a t i o n o f [C] / m o I L^{- 1} s^{- 1} 1. & 0.30 & 0.30 & 0.10 2. & 0.30 & 0.60 & 0.40 3. & 0.60 & 0.30 & 0.20 \end{matrix}$ $(a) R a t e = k [A]^{2} [B] (b) R a t e = k [A] [B]^{2} (c) R a t e = k [A] [B] (d) R a t e = k [A]^{2} [B]^{0}$

Compounds 'A' and 'B' react according to the following chemical equation. A(g)+2B(g)⟶2C(g) Concentration of either 'A' or 'B' were changed keeping the concentration of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction. ExperimentInitial Concentration of [A]/moIL−1Initial cooncentration of [B]/moIL−1Initial cooncentration of [C]/moIL−1s−11.0.300.300.102.0.300.600.403.0.600.300.20 (a)Rate=k[A]2[B] (b)Rate=k[A][B]2(c)Rate=k[A][B] (d)Rate=k[A]2[B]0

Answer»

Compounds 'A' and 'B' react according to the following chemical equation.

$A (g) + 2 B (g) ⟶ 2 C (g)$

Concentration of either 'A' or 'B' were changed keeping the concentration of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.

$\begin{matrix} E x p e r i m e n t & I n i t i a l C o n c e n t r a t i o n o f [A] / m o I L^{- 1} & I n i t i a l c o o n c e n t r a t i o n o f [B] / m o I L^{- 1} & I n i t i a l c o o n c e n t r a t i o n o f [C] / m o I L^{- 1} s^{- 1} 1. & 0.30 & 0.30 & 0.10 2. & 0.30 & 0.60 & 0.40 3. & 0.60 & 0.30 & 0.20 \end{matrix}$
$(a) R a t e = k [A]^{2} [B] (b) R a t e = k [A] [B]^{2} (c) R a t e = k [A] [B] (d) R a t e = k [A]^{2} [B]^{0}$

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