Q.1 order of N2 =3
Q.2 order of O3 = 1
Q.3 order of reaction= 3+1=4
Q.4 rate of reaction= 1.60*10^6M/s
Q.5 rate constant(K)=1.48M^-3s^-1
The rate of a certain reaction is given by the following rate law: rate=k [N_]*[0] Use...
The rate of a certain reaction is given by the following rate law: rate = k [12][H,] Use this information to answer the questions below. What is the reaction order in N2? DD What is the reaction order in H2? What is overall reaction order? At a certain concentration of N2 and H2, the initial rate of reaction is 0.860 M/s. What would the initial rate of the reaction be if the concentration of N2 were halved? Be sure your...
O KINETICS AND EQUILIBRIUM Using a rate law The rate of a certain reaction is given by the following rate law: rate =k[N][H] Use this information to answer the questions below. What is the reaction order in N2? DO What is the reaction order in H2? X 5 ? What is overall reaction order? At a certain concentration of N, and Hz, the initial rate of reaction is 2.0 x 105 M/s. What would the initial rate of the reaction...
The rate of a certain reaction is given by the following rate law: rate=k[NO] ?[02] Use this information to answer the questions below. What is the reaction order in NO? What is the reaction order in 02? What is overall reaction order? At a certain concentration of NO and O2, the initial rate of reaction is 73.0 M/s. What would the initial rate of the reaction be if the concentration of NO were doubled? Round your answer to 3 significant...
The rate of a certain reaction is given by the following rate law: rate = k [NO]2[O2] Use this information to answer the questions below 1. What is the reaction order in NO? ________ 2. What is the reaction order in O2? __________ 3. What is overall reaction rate? __________- 4. At a certain concentration of NO and O2, the initial rate of reaction is 9.0 x 105M / s. What would the initial rate of the reaction be if...
22. The rate law for the chemical reaction shown below has been determined experimentally: Rate = k[O3][CI]. What is the overall order of the reaction? 03(g) + Cl(g) → O2(g) + ClO(g) a. 3 b. 5 d. 2 8. The following data were obtained for the hypothetical reaction A+B → products. [A]o (M) 4.0 2.0 4.0 [B]. (M) 6.0 6.0 3.0 Initial Rate (M/s) 1.60 0.80 0.40 What is the overall order of this reaction? a. 3 b. 12 c....
Using an integrated rate law for a first-order reaction Consider this reaction 2H,PO.(ay) --P,03(aq) + 3H,0 (aq) At a certain temperature it obeys this rate law. rate= (0,0854 s [H, PO ] Suppose a vessel contains H, PO, a concentration of 1.49 M. Calculate the concentration of H, PO, in the vessel 7.70 seconds later. You may assume no other reaction is important Round your answer to 2 significant digits OM
At a certain temperature the rate of this reaction is second order in NH3 with a rate constant of 2.64·M−1s−1 , 2NH3g---> N2 g + 3H2 g Suppose a vessel contains NH3 at a concentration of 1.36M. Calculate the concentration of NH3 in the vessel 0.990 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits
A certain reaction is second order in N2 and first order in H2. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N2] [H2] initial rate of reaction 0.229 M 2.33 M 57.0 M/s 0.111 M 2.33 M __________M/s 0.0482 M 11.1 M ___________M/s
Some measurements of the initial rate of a certain reaction are given in the table below. [N2] [H2] initial rate of reaction 1.10 M 1.12 M 0.0454 M/s 1.10 M 0.528 M 0.0214 M/s 0.124M 1.12 M 0.000577 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....
some measurements of the initial rate of a certain reaction are given in the table below CO ADVANCED MATERIAL Deducing a rate law from Initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. N2] [H] initial rate of reaction 1.61 M 0.719 M 7.00 X 10M/s 1.61 M 0.113 M 173. M/s 0.710 M 0.719M 1.36 10 m/s Use this information to write a rate law for this reaction,...