Half-life equation for first-order reactions:where t₁/2is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹).To calculate the half-life, plug the value for k into the half-life equation and solve.What is the half-life of a first-order reaction with a rate constant of 7.80x10-4 s-¹?Express your answer with the appropriate units.888 st₁/2 =3.67x10-3 S-1||0.693kWhat is the rate constant of a first-order reaction that takes 189 seconds for the reactant concentration to drop to half of its initial value?Express your answer with the appropriate units.A certain first-order reaction has a rate constant of 1.90x10-3-¹. How long will it take for the reactant concentration to drop to of its initial value?Express your answer with the appropriate units.

Given that the half life of the first order reaction t1/2 = 0.693k rate constant given (k) :…

Half-life equation for first-order reactions: where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹). To calculate the half-life, plug the value for k into the half-life equation and solve. What is the half-life of a first-order reaction with a rate constant of 7.80x10-4 S-¹? Express your answer with the appropriate units. 888 s 11/2 3.67x10-3-1 = 0.693 k What is the rate constant of a first-order reaction that takes 189 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. A certain first-order reaction has a rate constant of 1.90x10-3-¹. How long will it take for the reactant concentration to drop to of its initial value? Express your answer with the appropriate units.

Half-life equation for first-order reactions: where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹). To calculate the half-life, plug the value for k into the half-life equation and solve. What is the half-life of a first-order reaction with a rate constant of 7.80x10-4 S-¹? Express your answer with the appropriate units. 888 s 11/2 3.67x10-3-1 = 0.693 k What is the rate constant of a first-order reaction that takes 189 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. A certain first-order reaction has a rate constant of 1.90x10-3-¹. How long will it take for the reactant concentration to drop to of its initial value? Express your answer with the appropriate units.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,Og) —CH,(g) +CO(g) Verify that this is a first-order reaction by plotting In[C,H,O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 52.0 75.0 97.0 135.0 k == min!
A chemical engineer is studying the rate of this reaction. 2N,0, (g) → 2N,O4g)+O2 (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds. Here's a graph of his data: 2 1.5 - 0.5 0. 0.2 0.4 0.6 0.8 1.2 t (s) (x) [°o°n]
A chemical engineer is studying the rate of this reaction. 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds. Here's a graph of her data: 2 5 t (s) [C1₂05] (M) 1.5 0.5 0 0
A first-order reaction has a rate constant of 3.6 x 10-3s-1. How many seconds does it take for the reaction to be 31.3% complete? (Report an integer)
A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻ because it is first order for I - . After you find the reaction order for S2O82⁻ you need to calculate k. S2O82⁻ (aq) + 3 I⁻ (aq) → 2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 ) 0.30 0.42 4.54 0.44 0.42 6.65 Rate = 120 M-2s-1 [S2O82⁻]2[I⁻] Rate = 195 M-3s-1 [S2O82⁻]2[I⁻] Rate = 86 M-2s-1 [S2O82⁻][I⁻] Rate = 23 M-1/2s-1 [S2O82⁻][I⁻] Rate = 36 M-1s-1 [S2O82⁻][I⁻]
The reactant concentration in a first-order reaction was 5.80×10−2 M after 40.0 s and 1.60×10−3 M after 70.0 s . What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
Calculate the rate constant (in units 1/M•min) for a second order reaction with a half life of 70.1 minutes and an initial concentration of 0.556 M
Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
Consider two different first order reactions, A → B and XY The first reaction has a half life of 30 minutes. The second reaction has a half life of 60 minutes. Which has a smaller rate constant? If both are started with 3 moles of their respective reactants, which reacts more quickly? A reaction with second order kinetics starts with a concentration of 10.0 M and is run for 30.0 seconds. If the value of k is 0.00900 M¹s¹ what is the new concentration?
Consider a first order reaction AB }A+ B If the reaction is 34% complete at the end of 39 s, what is the length of the half-life of this reaction in seconds? Use 2 significant figures in your answer. Do not include the unit.