Chemistry 132 Homework Chemical Kinetics and Equilibrium A certain first-order r
ID: 105026 • Letter: C
Question
Chemistry 132
Homework Chemical Kinetics and Equilibrium
A certain first-order reaction has a rate constant k = 1.6 x 10-3 s-1.
What is the half-life for the reaction?
The decomposition of NOCl, 2NOCl 2NO + Cl2, has k = 9.3 x 10-5 L mol-1s-1 at 100oC and k = 1.0 x 10-3 L mol-1s-1 at 130oC.
What is Ea for this reaction in kJ mol-1?
Use the data at 100oC to calculate the frequency factor.
The conversion of cyclopropane an anesthetic, to propylene has a rate constant
k = 1.3 x 10-6 s-1 at 400oC and k = 1.1 x 10-5 s-1 at 430oC.
(a)What is the activation energy in kJ/mol?
(b)What is the value of the frequency factor, A for this reaction?
(c)What is the rate constant for the reaction at 350oC?
The reaction of CO2 with water to form carbonic acid, CO2(aq) + H2O H2CO3(aq), has k = 3.75 x 10-2 s-1 at 25oC and 2.1 x 10-3s-1 at 0oC, what is the activation energy for this reaction in kJ/mol?
If a reaction has k = 3.0 x 10-4s-1 at 25oC and an activation energy of 100.0 kJ/mol, what will the value of k be at 50oC?
The decomposition of N2O5 has an activation energy of 103 kJ/mol and a frequency factor of 4.3 x 1013 s-1.
What is the rate constant for this decomposition at (a) 20oC and (b) 100oC?
Write the equilibrium law for each of the following reactions in terms of molar concentrations:
(a)2PCl3(g) + O2(g) = 2POCl3(g)
(b)2SO3(g) = 2SO2(g) + O2(g)
(c)N2H4(g) + 2O2(g) = 2NO(g) + 2H2O(g)
(d)N2H4(g) + 6H2O2(g) = 2NO2(g) + 8H2O(g)
(e)SOCl2(g) + H2O(g) = SO2(g) + 2HCl(g)
Write the equilibrium law for each of the following gaseous reactions in terms of molar concentrations:
(a)3CL2(g) + NH3(g) = NCl3(g) + 3HCl(g)
(b)PCl3(g) + PBr3(g) = PCl2Br(g) + PClBr2(g)
(c)NO(g) + NO2(g) + H2O(g) = 2HNO2(g)
(d)H2O(g) + Cl2O(g) = 2HOCl(g)
(e)Br2(g) + 5F2(g) = 2BrF5(g)
Write the equilibrium law for the reactions in Problem 7 in terms of partial pressures.
Write the equilibrium law for the reactions in Problem 8 in terms of partial pressures.
Write the equilibrium law for each of the following reactions in aqueous solution:
(a)Ag+(aq) + 2NH3(aq) = Ag(NH3) 2+(aq)
(b)Cd2+(aq) + 4SCN-(aq) = Cd(SCN)4-2(aq)
(c)HClO(aq) + H2O(l)= H3O+(aq) + ClO-(aq)
(d)CO3-2(aq) + HSO4-(aq) = HCO3-(aq) + SO4-2(aq)
A 345 mL container holds NH3 at a pressure of 745 torr and a temperature of 45oC. What is the molar concentration of ammonia in the container?
In a certain container at 145oC the concentration of water vapor is 0.0200 M. What is the partial pressure of H2O in the container?
Write the equilibrium law corresponding to Kc for each of the following heterogeneous reactions:
(a)2C(s) + O2(g) = 2CO(g)
(b)2NaHSO3(s) = Na2SO3(s) + H2O(g) + SO2(g)
(c)2C(s) + 2H2O(g) = CH4(g) + CO2(g)
(d)CaCO3(s) + 2HF(g) = CaF2(s) + H2O(g) + CO2(g)
(e)CuSO4 5H2O(s) = CuSO4(s) + 5H2O(g)
Write the equilibrium law corresponding to Kc for each of the following heterogeneous reactions:
(a)CaCO3(s) + SO2(g) = CaSO3(s) + CO2(g)
(b)AgCl(s) + Br-(aq) = Ag Br(s) + Cl-(aq)
(c)Cu(OH)2(s) = Cu+2(aq) + 2OH-(aq)
(d)Mg(OH)2(s) = MgO(s) + H2O(g)
(e)3CuO(s) + 2NH3(g) = 3Cu(s) + N2(g) + 3H2O(g)
Explanation / Answer
1)
we have:
k = 0.0016 s-1
use relation between rate constant and half life of 1st order reaction
t1/2 = (ln 2) / k
= 0.693/(k)
= 0.693/(1.6*10^-3)
= 433 s
Answer: 433 s
Only 1 question at a time please
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