33. The following data were obtained for the hypothetical reaction 2A+BD product
ID: 1019277 • Letter: 3
Question
33. The following data were obtained for the hypothetical reaction 2A+BD products. IAh M IBla(M 0.1 0.2 0.1 Initial Rate (Mis) 0.2 0.2 0.6 5 20 45 What is the overall order of this reaction? 34. The following reaction is investigated (assume an ideal gas misxture): 2N,O(g) + N,H,(g)3N(8)+ 2H,OUg) Initially there are 0.10 mol of N,O and 0.25 mol of Nala, in a 100-L container. If there are 0.062 mol of N,O at equilibrium, how many moles of N2 are present at A)1.9 x 10° B) 57 x 10° C) 1.1×10' D) 3.8 x10" E) none of these ny moles of Na are present at equilibrium? 35. For a certain second-order concentration of the reactant is 0.33 mol/L What is the rate constant for this reaction? A) 1.21 L(mol s) B) 0.40 L(mol s) C) 0.27 L(mol s) certain second-order decomposition reaction, the rate is 0.40 mol/(L. s) when the D) 0.83 L/(mol. s) E) 3.7L(mol s) 36. Exactly 1.0 mol NGO, is placed in an empty 1.0-.container and allowed to reach equilibrium described by the equation NO4g)2NO-(g) If at equilibrium the N204 is 380)% dissociated, what is the value of the equilibrium constant. K for the reaction under these conditions? A) 093 B) 123 C) 058 D) 11 E 0.23 37. A350-L vessel at 700 K initially contains HI(g) at a pressure of 3.60 atm; at equilibrium, it is found that the partial pressure of Ha(g) is 0.348 atm. What is the partial pressure of HI(g) at equilibrium? A) 0.348 atm B) 3.25 atm C) 3.60 atm D) 3.95 atm E) 290 atm 38. For the hypothetical reaction 2A+ BO 2C+ D, the initial rate of disappearance of A is 20 x 102 mol (L s). What is the initial rate of disappearance of B? A) 1.4 × 10" mol (L. s) B) 1.0 × 102 mold. . s) D) 4.0x 104 mol/(L s) E) 14x 102 mol (L. s) C) 80x 10* mol(L. s 39. In an experiment, 0.44 mol H2 and 0.44 mol Ia are mixed in a 1.00-L container, and the reaction forms HI. If K-49 for this reaction, what is the equilibrium concentration of HI? 1:(g)+Hg)2HI(g) A) 0059 M B) 0.77 MC) 0.68M D) 0.110 M E 085 M If K, = 0.132 for A2 + 2B -2AB, what is the value of K for the reaction A) 57.4 B) -0.132 C) 0.132 D) 3.79 E) 0.264 40.Explanation / Answer
1.
Let the rare –r be represented as –r = K[A]m[ B]n
where m and n are orders of reaction with respect to [A] and [B] respectively.
From experiment-1
5= K[ 0.2]m [0.1]n (1)
From experiment 2
20= K[0.2]m [0.2]n (2)
Eq.2/ Eq.1 gives 4= 2n , n=2
From experiment 3
45= K[0.6]m [0.1]n (3)
Eq.3/ Eq.1= 3m= 9, m =2
The overall order is = 2( order with respect to A ) + 2 ( order with respect to B)= 4 ( D is correct)
2.
For every 2 moles of N2O, 1 mole of N2H4 react to give 3 moles of N2 and 2 mole of H2O
Moles of N2O reacted = 0.1-0.062= 0.038 moles
2 mole of N2O gives 3 moles of N2
0.038 moles gives 0.038*3/2= 5.7*10-2 moles ( B is correct)
3.
3. For second order reaction
-rA= K[A]2
[A ] = concentration of reactant
0.40= K[0.33]2
K= 3.67 L/mol.s ( close answer is 3.71 /Mol.s
4.
Concentration of N2O4= 1/1 = 1M
Amount dissociated = 38%, amount of N2O4 remaining at equilibrium= 1-0.38= 0.62
Moles of N2O formed = 2*0.38= 0.76 moles, concentration = 0.76/1 =0.76M
Equilibrium constant for the reaction N2O4--à 2NO2, = [N2O]2/ [N2O4] =0.762/0.62=0.93 (A is correct)
5.
let x= parital pressure of H2 at equilibrium =0.348 atm
partial pressure of I2= 0.348 atm (since 2HI-à H2+I2)
Total pressure = 3.6= 0.348+0.348 + partial pressure of HI, partial pressure of HI= 2.9 atm ( E is correct)
6.
For the given reaction
-1/2 dCA/dt= dCD/dt ( A is decomposed and D is formed )
Given –dCA/dt= 2*10-2
dCD/dt= 2*10-2/2= 10-2M ( B is correct)
7.
Kc for the reaction H2(g) +I2(g) --> 2HI (g)
Kc= [HI]2/ [H2][I2]
Initially concentrations : H2= 0.44/1 =0.44M and I2= 0.44/1 =0.44
Let x= drop in concentration of H2 to reach equilibrium
At equilibrium [H2] = [I2] =0.44-x
[HI] =2x
Kc= (2x)2/ (0.44-x)2= 49, Taking square root , 2x/ (0.44-x)= 7
2x =7*(0.44-x), 9x= 7*0.44, x= 7*0.44/9 =0.34
[H I] =2*0.34= 0.68M ( C is correct)
8.
9. For the reaction A2 +2B-->2AB, Kc= [AB]2/ [A2] [B]2 = 0.132
Kc= [A2] [B]2/ [AB]2 =1/0.132 =7.6 (1)
For the reaction 4AB - >2A2 +4B,
Kc1= [A2]2 [B]4/ [AB]4= (Kc)2= (7.6)2= 57.76 ( A is correct)
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