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]o = 8.50 × 10 M, how long will it take for [A],= 3.40 × 10 M? min (b) Calculate the half-life of the reaction. min

Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first-order process to methane and ketene (CH2═C═O). At 600°C, the rate constant is 8.7 × 10−3 s−1. (a) What is the half-life of the reaction? Give your answer in scientific notation. (b) How long does it take for 38% of a sample of acetone to decompose?  (c) How long does it take for 81% of a sample of acetone to decompose? Give your answer in scientific notation.

The reaction 2A + 2B → M+ N has the rate law: Rate = k[A]². At 25°C, k = 0.0107 L mol-1 s1. If the initial concentrations of A and B are 0.314 M and 0.582 M, respectively Your answer is correct. (a) What is the half-life of the reaction? 297. seconds Hint Assistance Used Your answer is partially correct. (b) What will be the concentrations of A and B after 30.0 minutes? [A] = 0.0446 M [B] = i 0.048 ! M

Be sure to answer all parts. Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first- order process to methane and ketene (CH,=C=0). At 600°C, the rate constant is 8.7 x 103 s1. (a) What is the half-life of the reaction? Give your answer in scientific notation. x 10 (select) A (b) How long does it take for 42% of a sample of acetone to decompose? (c) How long does it take for 82% of a sample of acetone to decompose? Give your answer in scientific notation. x 10 (select) O S

In the presence  of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is (1.47x10^0)/s. Fe3+(aq) + SCN-(aq)  → Fe(SCN)2+(aq). What is the half-life, in seconds, of the reaction? Express your answer to three significant figures.

1a) Calculate the rate constant (with appropriate units) for a first order reaction which is 32.0% complete in 380 s. 1b) What is the value of the half-life of the reaction? 1c) How long will it take for the reaction to go to 76.0% completion?

Iodine atoms combine to form molecular iodine in the gas phase This reaction follows second-order kinetics and has the high rate constant 7.0 x 10°/M s at 23°C. If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min. (a) (b) Calculate the half-life of the reaction if the initial concentration of I is 0.60 M and if it is 0.42 M. B Strategy (a) I(g) + I(g) → 12 (8) (b) 1 1+1—h Page 589 The relationship between the concentrations of a reactant at different times is given by the integrated rate law. Because this is a second-order reaction, we use Equation (13.7). We are asked to calculate the half-life. The half-life for a second-order reaction is given by Equation (13.8).

The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(g) +SİH4(g)–→HI(g) +SIH3I(g) The activation energy is Ea = 83.2 kJ mol-1. At 269°C, the reaction rate constant is 3.49 L mols. (a) Calculate the Arrhenius factor A for this reaction. L mols1 (b) Calculate the rate constant for this reaction at 235°C. L molls1

The initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, k

She fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds. Here's a graph of her data: (W) [200³H] 2 1.5- 0.5 0 0 t(s) Use this graph to answer the following questions: What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in 11/2 = ☐ s S ☐ x10 H2CO3. Calculate the value of the rate constant k. k = ☐ Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of H2CO3 in the engineer's reaction vessel after 5.0 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in H2CO3. Round your answer to 2 significant digits. [H₂CO,] = M