JEE MAIN - Chemistry (2019 - 9th January Evening Slot - No. 18)
For the reaction, 2A + B $$ \to $$ products, when the concentrations of A and B both were doubled, the rate of the reaction increased from 0.3 mol L$$-$$1s$$-$$1 to 2.4 mol L$$-$$1s$$-$$1. When the concentration of A alone is doubled, the rate increased from 0.3 mol L$$-$$1s$$-$$1 to 0.6 mol L$$-$$1s$$-$$1.
Total order of the reaction is 4
Order of the reaction with respect to B is 2
Order of the reaction with respect to B is 1
Order of the reaction with respect to A is 2
Explanation
$$r = K{\left[ A \right]^x}{\left[ B \right]^y}$$
$$ \Rightarrow 8 = {2^3} = {2^{x + y}}$$
$$ \Rightarrow x + y = 3\,...(1)$$
$$ \Rightarrow 2 = {2^x}$$
$$ \Rightarrow x = 1,y = 2$$
Order w.r.t. A = 1
Order w.r.t. B = 2
$$ \Rightarrow 8 = {2^3} = {2^{x + y}}$$
$$ \Rightarrow x + y = 3\,...(1)$$
$$ \Rightarrow 2 = {2^x}$$
$$ \Rightarrow x = 1,y = 2$$
Order w.r.t. A = 1
Order w.r.t. B = 2
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