Equal volumes of two equimolar solutions of reactants A and B are mixed and the reaction A + B → C occurs. At the end of 1 hr, A is 75 % reacted. What percentage of A will be left unreacted at the end of 3 hr if the reaction is: (a) First order in A and zero order in B (b) First order in A and first order in B

9:53 AM Tue Nov 21 Question 18 of 20 Step 1 (slow) H₂O2(aq) + (aq) H2O(l) + IO-(aq) Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I¯(aq). What is the rate law for this reaction? Step 2 (fast) H₂O2(aq) + 10 (aq) → H₂O(l) + O2(g) + (aq) A) rate= K[H₂O₂] B) rate= K[H₂O₂]² C) rate= K[H₂O₂] [1] D) rate = K[H₂O₂] [10] E) rate = K[H₂O₂]²[1]/[H₂O] Tap here or pull up for additional resources 36% Submit

The reaction A(aq) ---> B(aq) + C(aq) is a first order reaction. The half-life of A(aq) is 93.4 s at 25.0oC and its half-life is 71.7 s at 45.0oC. What is its half-life (in s) at 65.0oC?

The decomposition of ammonia is zero order process is with a half-life of 28.3 seconds at a certain temperature. If the pertinent rate constant is 0.00207 M.s1, what was the initial reactant concentration? The half-life of a zero-order reaction is concentration-independent (A) (B) (C) (D) (E) 17.1 M 0.0353 M 0.00207 M 0.117 M

a) The reaction A(ag) → B(aq) is first-order with respect to A(aq). The concentration of A(aq) after 100.0 s of reaction is 0.555 M. The concentration of A(aq) after a further 400.0 s (500.0 s total) is 0.333 M. What will be the concentration of A(aq) after a further 500.0 s (1000.0 s total)? What is the half-life of the reaction? The temperature is 25.0 °C throughout the reaction. b) The reaction 2 A(aq) → B(aq) is second-order with respect to A(aq). When the concentration of A(ag) is 0.150 M and the temperature is 25.0 °C, the reaction rate is 0.1350 M/s. If we increase the concentration of A(aq) to 0.450 M and lower the temperature to 5.0 °C, the rate of reaction becomes 0.0300 M/s. What is the activation energy for this reaction?

12.) The reaction: 2NO(g) + Cl₂ (3) 20NCI (3) is second order in NO), first order in Cl₂(3), and third order overall. Compare the initial vale of reachon. mixture. OF 0.02 mol mol with (a) the rate of the reaction when half of the NOA) has been consumed, of a OF NO) and 0.02 of cl₂g in a one-liter container (g) (b) the rate of the reaction when half of the Clz) has been consumed, (c) the rate of the reaction when two-thirds of the NO(g) has been consumed, (d) the initial rate of a mixture OF 0.04 mol OF NO) and 0.02 mol OF Cl₂ ) in one-liter container

Determine the ratio of the times at which a chemical reaction is 50% and 75% reacted, t½ t¼, for a reaction of a) zero order b) first order c) second order

Given the reaction  2N2O(g) → 2N2(g) + 1O2(g)  Is a first order reaction with a half-life of 3580 sec. If the initial concentration of N2O is 0.0255M, what is the concentration, in mol/L, of N2O after exactly 100 minutes?

The reaction: NO (g) + O3 (g) —> NO2 (g) + O2 (g) Is thought to be a second-order reaction with respect to O3. You start with [O3] = 0.250 M. After 125 s you find that the [O3] has dropped to 0.145 M. A) Assuming the reaction is second order, determine the value and units of the rate constant.  B) Determine the half-life of the reaction.  C) Calculate [O3] after 195 seconds.

The decomposition of sulfuryl chloride (SO2CI2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 10-2 s-1. (a) If we begin with an initial SO2Cl2 pressure of 335 torr, what is the pressure of this substance after 61 s? 22.40 is wrong. Incorrect: Your answer is incorrect. torr (b) At what time will the pressure of SO2Cl2 decline to one eighth its initial value? 26.20 is wrong Incorrect: Your answer is incorrect. s By what factor will the pressure of sulfuryl chloride decrease after 8 half lives? Note: The answer wants this value: (335 torr)/value = final pressure after decay 128 is wrong. Incorrect: Your answer is incorrect. value