3A+4B→2C is found to be second order with respect to A and the rate constant for the reaction is k = 2.98* 10^ {-9}k=2.98∗10^−9 \frac{L}{mole\cdot\sec}mole⋅secL​. If the initial concentration of A is 0.89 M0.89M how much many seconds will be required for the concentration of A to reach 0.65 M0.65M   you can input your answer as a whole number

The reaction A→ B is second order and has a rate constant k = 0.0136 M1s1. Determine how long it will take, in s, for the concentration of A to fall to 0.135 M if the initial concentration was 0.540 M.

A reaction 2 A → P has a second-order rate law with kr = 4.30 × 10−4 dm3 mol−1 s−1. Calculate the time required for the concentration of A to change from 0.210 mol dm−3 to 0.010 mol dm−3.

Please write every step as clear as possible so I can properly understand

2) Use the data below to determine the rate law and the value of k for the following reaction H2O2 (aq) + 3 I (aq) + 2H* (aq) →13° (aq) + H20 (1) Experiment [H20z] (M) [F] (M) [H*] (M) Initial Rate 0.0390 0.0470 0.0309 5.149 x 10-6 0.0779 0.0470 0.0309 1.030 x 10-5 2.059 x 10-5 5.149 x 10-6 3 0.0390 0.0939 0.0309 4 0.0390 0.0470 0.0620

the rate of decomposition of hydrogen peroxide in dilute sodium hydroxide at room temperature is as follows: 2H2O2(aq)-> 2H2O(l) +O2(g). the reaction is a first-order in H2O2. The rate constant for the decomposition of H2O2 at 20oC is 1.8x10-5 s-1, and the initial concentration of H2O2 is 0.80 mol L-1. (i)What is the concentration of H2O2 after 8.0hours? (ii) how long will it take for the concentration of H2O2 to drop to 0.10M? (iii) how long will it take for 75% of the H2O2 to decompose? (iii)

At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.00554M^−1.s^−1: H2CO3aq--->H2O(aq) + CO2(aq) Suppose a vessel contains H2CO3 at a concentration of 0.830M. Calculate how long it takes for the concentration of H2CO3 to decrease to 24.0% of its initial value. You may assume no other reaction is important. Round to 2 significant digits.

For a zero-order reaction with a starting concentration of 100mM A and a rateconstant of k=.0002 mol/s how long will it take for the reaction to proceed 25mM?

At a certain temperature, this reaction follows second-order kinetics with a rate constant of 0.372M−1*s−1: 2HIg->H2(g)+I2(g) Suppose a vessel contains HI at a concentration of 0.340M. Calculate how long it takes for the concentration of HI to decrease by 78.0%. You may assume no other reaction is important. Round your answer to 2 significant digits.

The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O,(g) 2N₂O(g) + O₂(g) Determine graphically the activation energy for the reaction. Round your answer to 2 significant digits. |*(-¹) T(K) k 303. 308. 313. 318. 323. 3.48 × 10 5 1.32×10 4 5.04 104 1.52 × 10-3 4.80 × 10-3 Note: Reference the Fundamental constants table for additional information. kJ mol X