7. A solution of A is mixed with an equal volume of a solution of B containing the same number of moles, and the reaction A+ B C occurs. At the end of 30 minutes, A is 50% reacted. How much of A will be left unreacted at the end of sixty minutes if the reaction is a. zeroth-order in both [A] and (B] b. first-order in [A] and zeroth-order in [B] c. first order in both [A] and [B]

What percentage of the initial amount of S02Cl2 2ilk remain after 2.25 hours?

The rate constant for a second-order reaction is 0.13 M1s1. If the initial concentration of reactant is 0.26 mol/L, it takes s for the concentration to decrease to 0.19 mol/L. O 5.3 O 0.18 O 11 O 1,4 O 0.017

Consider the first-order reaction shown below. The yellow spheres represent the reactant, A. The blue spheres represent the product, B. A B t=0 s t = 1.00 s

Many drugs decompose in blood by a first-order process. Two tablets of aspirin supply 0.60 g of the active compound. After 30 min, this compound reaches a maximum concentration of 2 mg/100 mL of blood. If the half-life for its breakdown is 90 min, what is its concentration (in mg/100 mL) 4.5 h after it reaches its maximum concentration?

The decomposition of a chemical follows the Zero order with a rate constant, k = 0.00543 M/s. If the initial concentration of the reactant is 2.32. what is the concentration after 900 seconds?. The decomposition of a chemical is in the second order with a rate constant, k = .0123 M-1min-1. If the initial concentration of the reactant is 0.765 M. What is the concentration after 15 minutes.

You have a second-order reaction for B which has an initial concentration of 30.00 moles in 15.00 L. If this process has a reaction constant k = 1.90x10-6 M-1s-1 What is the half-life of this reaction in second? In minutes? What is the concentration after the first half-life? What is the concentration after 5 half-lives? What is the concentration after 3.00x104 seconds? (hint: use the integrated rate equations!)

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?

The rate constant for this zero-order reaction is 0.0240 M •s= at 300 °C. A products > How long (in seconds) would it take for the concentration of A to decrease from 0.890 M to 0.270 M? t = S