Practice ProblemATTEMPT
The reaction
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Chemistry
- A reaction which is of first order w.r.t reactant A, has a rate constant 0.6 min [4]=0.5 mol L¹, when would [4] reach the value of 0.05 mol L-¹ If we start with (a) 0.384 min (b) 0.15 min (c) 3 min (d) 3.84 minarrow_forwardBe sure to answer all parts. The reaction 2A → B is second order in A with a rate constant of 33.5 M−1 · s−1 at 25 ° C. (a) Starting with [A]0 = 0.00801 M, how long will it take for the concentration of A to drop to 0.00180 M? s (b) Calculate the half-life of the reaction for [A]0 = 0.00801 M. s (c) Calculate the half-life of the reaction for [A]0 = 0.00289 M.arrow_forward2 attempts left Be sure to answer all parts. The reaction 2A → B is second order with a rate constant of 51.0/M min at 24°C. (a) Starting with [A]0 = 8.70× 10−3 M, how long will it take for [A]t = 3.00 × 10−3 M? min (b) Calculate the half-life of the reaction. minarrow_forward
- (a) For a generic second-order reaction A--->B, whatquantity, when graphed versus time, will yield a straightline? (b) What is the slope of the straight line from part(a)? (c) Does the half-life of a second-order reaction increase,decrease, or remain the same as the reactionproceeds?arrow_forwardFor a second-order reaction, the half-life is equal to a) t1/2=0.693/k b) t1/2=k/0.693. c) t1/2=1/k[A]o d) t1/2=k e) t1/2=[A}o/2karrow_forwardConsider a reaction which is 2nd-order in A (•) and 1st-order in B (0): A+ B C. What are the relative rates of this reaction in the vessels shown below arranged from slowest to fastest? Each vessel has the same volume. 7. (1) (II) (II) (IV) (a) IIIarrow_forwardThe radioactive decay of a certain isotope of lead is a first-order process that has a half-life of 242 minutes at a certain temperature. At this temperature, what percentage of the original concentration will be left after 45.0 minutes? (A) 0.29 % (B) 1.29 % (C) 87.9 % (D) 81.4 % (E) 18.6 %arrow_forwardConsider the second-order decomposition of A under the following conditions: The initial concentration of A is 0.161 M and after 117 s the concentration has decreased to 0.111 M. (a) What is the value of the rate constant k? 4.0 M-1*s-1 (b) What is the half-life of the reaction? 4.0arrow_forward(a) For the generic reaction A ---> B. If this is a first-order reaction, what quantity when graphed versus time will yield a straight line? (b) how can you calculate the rate constant for the first-order reaction from the graph you made in part (a)? Group of answer choices A.) (a) a graph on log[A] versus time yields a straight line for a first-order reaction. (b) the slope of the straight line. B.) (a) a graph on 1/[A] versus time yields a straight line for a first-order reaction. (b) the slope of the straight line. C.) (a) a graph on [A] versus time yields a straight line for a first-order reaction. (b) the slope of the straight line. D.) (a) a graph on ln[A] versus time yields a straight line for a first-order reaction. (b) the negative slope of the straight line.arrow_forwardFind the natural lifetime in seconds for first-order reactions corresponding to *(a) k = 0.497 s-1. (b) k = 6.62 h-1. *(C) [A]0 = 3.16 M, and [A]t = 0.496 M at t = 3876 s. (d) [P]' = 0.176 M, and [P]t = 0.0423 M at t = 9.54 s (assume 1 mol of product is formed for each mol of analyte reacted). *(e) half-life, t1/2, = 26.5 years. (f) t1/2 = 0.583 s.arrow_forward6. The second-order reaction 2 NO, 2 NO + 0 has a rate constantk 0.63 M's', If the initia. concentration of NO, is 0.100 M, what is the concentration after 1.50 sP () 0.039 M (b) 0.055 M (c) 0,068 M (d) 0.091 M tome ot 625 K with a first-order ratearrow_forwardWhat is the order of a reaction with respect to a reactant "A" if a plot of ln[A] vs time is linear? Group of answer choices A) first order B) zero order C) second orderarrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
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