Chemistry — mixed

At 518^oC the rate of decomposition of a sample of gaseous acetaldehyde initially at a pressure of 363 Torr, was 1.00 Torr s^–1 when 5% had reacted and 0.5 Torr s^–1 when 33% had reacted. The order of the reaction is

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.

For kinetic study of the reaction of iodide ion with $$\mathrm{H}_{2} \mathrm{O}_{2}$$ at room temperature : (A) Always use freshly prepared starch solution. (B) Always keep the concentration of sodium thiosulphate solution less than that of KI solution. (C) Record the time immediately after the appearance of blue colour. (D) Record the time immediately before the appearance of blue colour. (E) Always keep the concentration of sodium thiosulphate solution more than that of KI solution. Choose the correct answer from the options given below :

A student has studied the decomposition of a gas AB$$_3$$ at 25$$^\circ$$C. He obtained the following data. .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} p (mm Hg) 50 100 200 400 relative t$$_{1/2}$$ (s) 4 2 1 0.5 The order of the reaction is

For a chemical reaction $$\mathrm{A}+\mathrm{B} \rightarrow$$ Product, the order is 1 with respect to $$\mathrm{A}$$ and $$\mathrm{B}$$. .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} .tg .tg-amwm{font-weight:bold;text-align:center;vertical-align:top} $$\mathrm{Rate}$$ $$\mathrm{mol~L^{-1}~S^{-1}}$$ $$\mathrm{[A]}$$ $$\mathrm{mol~L^{-1}}$$ $$\mathrm{[B]}$$ $$\mathrm{mol~L^{-1}}$$ 0.10 20 0.5 0.40 $$x$$ 0.5 0.80 40 $$y$$ What is the value of $$x$$ and $$y$$ ?

If half-life of a substance is 5 yrs, then the total amount of substance left after 15 years, when initial amount is 64 grams is

The integrated rate equation is Rt = log C₀ - log C_t . The straight line graph is obtained by plotting

Units of rate constant of first and zero order reactions in terms of molarity M unit are respectively

For the reaction system: 2NO(g) + O₂(g) $$\to$$ 2NO₂(g) volume is suddenly reduce to half its value by increasing the pressure on it. If the reaction is of first order with respect to O₂ and second order with respect to NO, the rate of reaction will

In a first order reaction, the concentration of the reactant decreases from 0.8 M to 0.4 M in 15 minutes. The time taken for the concentration to change from 0.1 M to 0.025 M is