+ d. What is the rate of this reaction between 20.0 and 50.0 seconds? Use the balanced equation C3H,(g) +50₂(g) →3CO₂(g) + 4H₂O(g) to rank the substances in order of slowest to fastest rate of change in a given time interval. Fastest 3₂ e. Slowest

Consider the reaction below at 100oC  T2U (g)  ⟶⟶ 2 T (g)  + U (g)  When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, A. Which is the rate law of this reaction? B.  which is the numerical value of the specific-rate constant, k, for this reaction?  C. Which are the units for the specific rate constant, K? D. At whic rate is T generaten when [T2U] is 0. 111 M? E. if given an initial reactant concentration [T2U]o = 0.250 M, what is [T] after 15 minutes have elapsed?

A chemistry graduate student is studying the rate of this reaction: 2HI (g) → H₂ (g) +1₂ (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [HI] 0.0400M 0.0199M 0.20 0.0133 M 0.30 0.00994M 0.40 0.00795 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 X Ś

Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A]2 where k= 1.45 ×10-2 M-1s-1 at a particular temperature. If the initial [A] = 0.300 M, what will be the concentration of A remaining after 3.00 minutes?  0.168 M 0.0221 M 0.296 M 0.287 M

Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.55M 0.638M 14.0M/s 0.601 M 0.638M 2.10M/s 1.55M 1.92M 127.M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 ▬ x10 X 00 5

Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.85M 0.849 M 59.0 M/s 1.85M 0.188M 2.89 M/s 8.12M 0.849 M 259. M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k = k ☐x10 •

A chemistry graduate student is studying the rate of this reaction: H₂CO3 (aq) → H₂O (aq) + CO₂ (aq) He fills a reaction vessel with H₂CO3 and measures its concentration as the reaction proceeds: time (seconds) 0 10. 0.0334M 20. [H₂CO3] 0.100M 30. 0.0200M 0.0143 M 40. 0.0111 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X

Consider this reaction.    2A             B     It obeys the rate law:    rate =   k [A] 2   and  k = 0.188 M -1 s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? Consider this reaction.    2A             B     It obeys the rate law:    rate =   k [A] 2   and  k = 0.188 M -1s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? 793 s 8.87 s 182  s 9.48 x 103 s 79.1 s 3.07 x 10-3 s 1.50 x 109 s 5.22  x 10-2 s

The rate of a certain reaction is given by the following rate law: rate =k| N,| H2 -k[N;][H+]° Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.620 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 24.0 M / s when [N2] = 1.5 M and [H2] = 0.16 M. Calculate the value of the k = |M -2 -1 •S rate constant. Round your answer to 2 significant digits.

For the reaction shown below, the instantaneous change in concentration of NO(g) is 1.4 mol/L.s. 2NO(g) + Cl₂(g) →→ 2NOCI(g) What is the rate at which Cl₂(g) is consumed and the rate at which NOCI(g) is formed at this time?