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How the rate changes when concentrations, pressure or volume change

This type of question, asked 5 times: 5 Apr 2024, 9 Apr 2024, 28 Jan 2025, 4 Apr 2025, 22 Jan 2026 S1. All 5 questions below, oldest first.

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  1. Question 1

    5 Apr 2024

    147
    Consider the following single step reaction in gas phase at constant temperature.
    2 A(g)+B(g)→C(g)2{\text{ }A}_{(g)}+B_{(g)}\rightarrow C_{(g)}
    The initial rate of the reaction is recorded as r1r_{1} when the reaction starts with 1.5 atm1.5\text{ }atm pressure of AA and 0.7 atm pressure of B. After some time, the rate r2r_{2} is recorded when the pressure of CC becomes 0.5 atm0.5\text{ }atm. The ratio r1:r2r_{1}:r_{2} is _____ ×10−1\times10^{- 1}. (Nearest integer)

  2. Question 2

    9 Apr 2024

    52
    Given below are two statements: Statement I: The rate law for the reaction A+B→CA + B \rightarrow C is rate (r)=k[A]2[ B](r) = k\lbrack A\rbrack^{2}\lbrack\text{ }B\rbrack. When the concentration of both AA and BB is doubled, the reaction rate is increased " xx " times. Statement II: The figure is showing "the variation in concentration against time plot" for a " yy " order reaction. The value of x+yx + y is. _______

  3. Question 3

    28 Jan 2025

    101
    consider the elementary reaction
    A( g)+B( g)→C( g)+D( g)A(\text{ }g) + B(\text{ }g) \rightarrow C(\text{ }g) + D(\text{ }g)
    If the volume of reaction mixture is suddenly reduced to 13\frac{1}{3} of its initial volume, the reaction rate will become ' xx ' times of the original reaction rate. The value of xx is :

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  4. Question 4

    4 Apr 2025

    33
    Rate law for a reaction between AA and BB is given by R=k[ A]n[ B]mR = k\lbrack\text{ }A\rbrack^{n}\lbrack\text{ }B\rbrack^{m}If concentration of A is doubled and concentration of BB is halved from their initial value, the ratio of new rate of reaction to the initial rate of reaction (r2r1)\left( \frac{r_{2}}{r_{1}} \right) is.

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  5. Question 5

    22 Jan 2026 S1

    37
    A → products (First order reaction). Three sets of experiment were performed for a reaction under similar experimental conditions. Run 1⇒100 mL1 \Rightarrow 100\text{ }mL of 10 M solution of reactant A Run 2⇒200 mL2 \Rightarrow 200\text{ }mL of 10 M solution of reactant A Run 3⇒100 mL3 \Rightarrow 100\text{ }mL of 10 M solution of reactant A+A + 100 mL of H2OH_{2}O added. The correct variation of rate of reaction is

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