In some reactions, the spatial orientation of the reactant molecules is a very important factor in determining the rate of the reaction.   In other reactions, it is not.  Which theory would you use to explain these two statements?  And why?

Some measurements of the initial rate of a certain reaction are given in the table below. H2 12 initial rate of reaction 1.89 M | 0.790м 9.00 x 10°M/s 2.27 x 10°M/s 1.78 x 10° M/s 1.89 M | 0.199м |0.373 М 0.790м 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 =

Some measurements of the initial rate of a certain reaction are given in the table below. [N2] H2 initial rate of reaction 1.02M 1.73М 0.0437M/s 1.02M |6.60М 0.167 M/s 0.333 M 1.73М 0.00466M/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 =

A chemistry graduate student is studying the rate of this reaction: 2Cl2O5(g)-->2Cl2(g)+5O2(g) She fills a reaction vessel with Cl2O5 and measures its concentration as the reaction proceeds: time(minutes) Cl2O5 0 1.00M 10. 0.428M 20. 0.272M 30. 0.200M 40. 0.158M Use this data to answer the following questions. Write the rate law for this reaction. rate =k   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. k=

A chemistry graduate student is studying the rate of this reaction: 2C1,0, (3) – 2Cl, (g) +50, (g) She fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds: time [CLO,] (seconds) 1.00 M 10. 0.666 M 20. 0.443 M 30. 0.295 M 40. 0.196 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k O Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.

A chemistry graduate student is studying the rate of this reaction: NH4OHaq→NH3aq+H2Oaq She fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds time(seconds) NH4OH 0 0.0700M 10. 0.0370M 20. 0.0196M 30. 0.0103M 40. 0.00547M Use this data to answer the following questions. Write the rate law for this reaction. rate =k   Calculate the value of the rate constant k.Round your answer to 2significant digits. Also be sure your answer has the correct unit symbol. =k

A certain reaction is known to have an activation energy E-41.0 kJ/mol. Furthermore, the rate of this reaction is measured at 347. K and found to be 6.7 × 10² M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is lowered by 10% from 347. K to 312. K. The rate will choose one How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is added, which has the effect of lowering the activation energy by 10%, from 41.0 kJ/mol to 36.9 kJ/mol. The rate will choose one How will the rate of the reaction change? X Ś ?

Given the equation:  rate = k[H2O2]m[I-]n Which of the following statements is (are) true about the orders, m and n? a. m and n are equal to each other in all cases b. m and n are independent from the molar coefficients of the reactants in the balanced chemical equation c. m and n must be determined by experiment d. m and n are equal to the molar coefficients of H2O2 and I- in the balanced chemical reaction, respectively

Some measurements of the initial rate of a certain reaction are given in the table below. N2||H2 initial rate of reaction 0.673 M 1.18M 2.00 x 10°M/s 0.673 M 1.49M 3.19 x 10°M/s 0.305 M 1.18M 4.11 × 10*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 %3D |x10 k = 0

Some measurements of the initial rate of a certain reaction are given in the table below. [H,] I initial rate of reaction 0.283 M 1.65 M 0.858 M/s 0.283 M 2.21 M 1.15 M/s 0.125 M 1.65 M 0.379 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.