The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N2O5 and first order overall.  The rate constant for the reaction at 70.oC is 6.82x10-3 s-1.  The reaction is started with 0.300 mol of N2O5 in a 0.500L container. What is the rate law for this reaction?

The first-order rate constant for the decomposition of C2H5Cl, C2H5Cl(g)  C2H4(g) + HCl(g) at 27 oC is k = 7.27e-30 s-1. Suppose we start with 0.0845 mol of C2H5Cl in a volume of 4.9 L. How many moles of C2H5Cl will remain after 1.24e+27 min?

The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl]. At 550°C, k = 3.2 x 10-2 sec-1. What is the half-life for this reaction? What was the initial concentration of ethyl chloride if after one minute, 0.01 M remains?

A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 2.55 x 108 s at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days) Round your answer to 2 decimal places.

The decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 Kis 4.5×10−2s−1. A)If we begin with an initial SO2Cl2 pressure of 460 torr, what is the partial pressure of this substance after 63 s? B) At what time will the partial pressure of SO2Cl2 decline to one-third its initial value?

The thermal decomposition of sulfuryl chloride to sulfur dioxide and chlorineSOCl(g)  SO(g) + Cl(g)is a first order reaction with a half-life of 2.3010 seconds. For this reaction what is the numerical value of k, the rate constant, in s?

At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S

The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N₂05 and first order overall. The rate constant for the reaction at 70.°C is 6.82x10-3 s-1. The reaction is started with 0.300 mol of N205 in a 0.500L container. What will the concentration of N2O5 be after 1.50 minutes? O a. 0.594M O b. 0.438M O c. 0.297M O d. 0.325M O e. 0.162M O f. 0.253M

for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction

Iodine atoms will combine to form I2 in liquid hexane solvent with a rate constant of 1.5×1010L/mol⋅s. The reaction is second order in I . Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of I2. Suppose a flash of light creates an initial [I] concentration of 1.00×10−2 M How long will it take for 97% of the newly created iodine atoms to recombine to form I2? Express your answer using two significant figures.