Rate law
Rate = K[A]^x[B]^y[C]^z
3 = K(0.273)^x(0.763)^y(0.4)^z -------->
1
9 = K(0.819)^x(0.763)^y(0.4)^z
----------> 2
12 = K(0.273)^x(1.526)^y(0.4)^z
----------> 3
6 = K(0.273)^x(0.763)^y(0.8)^z
----------> 4
equation 1 divide by equation 2
3/9 =
K(0.273)^x(0.763)^y(0.4)^z/K(0.819)^x(0.763)^y(0.4)^z
0.33 = (0.273/0.819)^x
(0.33)^1 = (0.33)^x
x = 1
equation 1 divide by equation 3
3/12 =
K(0.273)^x(0.763)^y(0.4)^z/K(0.273)^x(1.526)^y(0.4)^z
0.25 = (0.763/1.526)^y
(0.5)^2 = (0.5)^y
y = 2
equation 1 divide by equation 4
3/6 =
K(0.273)^x(0.763)^y(0.4)^z/K(0.273)^x(0.763)^y(0.8)^z
0.5 = (0.4/0.8)^z
(0.5)^1 = (0.5)^z
z = 1
Rate law
Rate = K[A]^1[B]^2[C]^1
Rate = K[A][B]^2[C] >>>>>answer
Q16.
SOCl2(g) ---------> SO2(g) + Cl2(g)
Dn = (1+1) -1 = 1
Kp = Kc(RT)^Dn
1.23*10^-6 = Kc(0.0821*500)^1
Kc = 1.23*10^-6/(0.0821*500) = 3*10^-8
3.00*10^-8 >>>>answer
Q17.
K = 0.693/t1/2
= 0.693/0.2
= 3.47s^-1 >>>>answer
Q18.
molarity of CO = no of moles/volume in L
= 3/0.5 =6M
molarity of H2O = no of moles/volume in L
= 3/0.5 =6M
------- CO(g) + H2O(g) ------> H2(g) + CO2(g)
I------ 6--------6 -----------0 ---------0
C------ -x ------ -x --------- +x -------+x
E------ 6-x ---- 6-x --------- +x -------+x
Kc = [H2][CO2]/[CO][H2O]
16 = x*x/(6-x)(6-x)
16 = (x/6-x)^2
4 = x/6-x
4(6-x) = x
[CO2] =x = 4.8M
4.80M >>>>answer
we - Google Given the following data, determine the rate law for the following reaction 2A+B+2C...
Part A The data in the table below were obtained for the reaction: A + B → P Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83 3 0.819 0.763 25.47 The magnitude of the rate constant is ________. The data in the table below were obtained for the reaction: A + B → P Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83...
Calculate the rate coefficient (mol-1 dms-2) for the following reaction: A+B → Products Experiment [A] (mol dm-3) 0.273 0.273 0.819 [B] (mol dm3) 0.763 1.526 0.763 Initial Rate(mol dm-3 s) 2.83 2.83 25.47 37.97 0.278 13.2 42.0
7. Given the following data for the reaction: NOrg) Expt.TAIIM +1/2 CHE)-NOCU8 BIM 0273 0.819 0.273 0.273 0.763 1526 0.763 0.400 0400 0.800 3.0 9.0 12.0 (a) Calculate the order with respect to each reactant. Om, n.p) 6.0 (b) Calculate k. (3 pts) (c) Write the rate law. (3 pts) 8. The reaction of NO with H2 is thought to occur in three elementary steps: NO + H2N+H2O (slow) N+NO N20 N20 +H2N2+H20 (fast) (a) Identify the reaction intermediate )....
The data below were obtained for the reaction A + B —> P Experiment number [A] (M)) [B] (M) Initial rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83 3 0.819 0.763 25.47 (C) What is the overall order of the reaction? (D) Write the rate law for this reaction. (E) Please calculate the rate constant for the reaction.
The data below were obtained for the reaction A + B —> P Experiment number [A] (M)) [B] (M) Initial rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83 3 0.819 0.763 25.47 (A) What is the order of the reaction with respect to A? (B) What is the order of the reaction with respect to B? (C) What is the overall order of the reaction?
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are A = 0.076 M B = 0.829 M If K = 3.32, find the concentration of C and report it in M units. B.) Cu (s) + 2 Ag+ ⇋ Cu2+ (aq+) + 2 Ag(s) K = 7.88 x 104 PbCl2 (s) ⇋ Pb2+ (aq) + 2 Cl- (aq) K = 2.4 x 10-4 AgI (s) ⇋ Ag+ (aq) + I- (aq) K =...
2. For the reaction: A(g) +B(g) = 2C(g) K = 1.0 x 10-5 at 25°C When equilibrium was reached at 25°C, the equilibrium concentrations of the reactant gases were: [A] = 2.5 x10-2M [B] = 2.0 x 10- M Calculate the equilibrium concentration of the product gas C? 3. At a certain temperature the reaction has an equilibrium constant of 0.400. CO(g) + H2O(g) = CO2(g) + H2(g) When 1.50 mol of carbon dioxide gas and 1.50 mol of hydrogen...
For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 1 0.015 M 0.200 M 3.67 x 10^-6 20.030 M 0.200 M 7.33 x 10^-6 30.015 M 0.400 M 1.47 x 10^-5 The special rate constant k = A 1.2 x 10^-3 (1/M.sec) 9.2 x 10^-4 (1/M-sec) C 1.6 x 10^-3 (1/M-sec) 6.1 x 10^-3 (1/M^2-sec) E 8.2 x 10^-3 (1/M^2-sec)
2 NO (9) 1. (2 pts) Use the following experimental data to write a Rate Law for this reaction. Show your work and draw a box around your final answer. + Cl2() + 2 NOCG) [NO] (M) (C12) (M) Initial Rate (Mis) 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 0.50 2. (2 pts) Consider this two-step mechanism for a reaction: Step 1: 2 NO (9) + 2 H2 (9) ** N2 () + H2O2() SLOW Step 2: H2020) +...
[A] (2) Consider this reaction: 2A + 2B → 2C+D (2.5 pts) [B] Initial Rate(M/s) (a) Write the rate law for this reaction 0.400 0.0100 5.90 x 10-6 (6) Calculate the rate constant. Include Units. 0.400 0.0400 9.44 x 105 (c) Is the reaction in an elementary reaction? Explain 0.400 0.0800 3.78 x 10-4 your answer in a sentence. 0.800 0.0600 2.12 x 10-4 (3) Here is a reaction: A products (1.5 pt) 0.800 0.0400 9.44 x 10-5 (3a) How...