reaction: Cu^2+ + 4NH3 yields Cu(NH3)4^2+ What is the rate for each trial? What
ID: 512579 • Letter: R
Question
reaction: Cu^2+ + 4NH3 yields Cu(NH3)4^2+
What is the rate for each trial?
What is the rate law expression in general form?
Determine order with respect to copper?
Determine order with respect to ammonia?
What is the overall order?
Determine the rate law constant for this reaction?
What is the complete rate law expression for this reaction?
What is the energy of activation for this reaction?
What is the Arrhenius factor at room temperature?
How many steps are in this reaction?
Write a balanced reaction for each elementary step?
Which is the rate limiting step?
trial Concentration of Cu^2+ (M) Concentration of NH3 (M) Temp (C) Time (sec) Rate ([NH3]/time) 1 0.010 0.030 25 428 ? 2 0.010 0.060 25 424 ? 3 0.020 0.030 25 210 ? 4 0.010 0.030 125 35 ?Explanation / Answer
1. answer : rate of reaction = -d[Cu]2+/dt =-1/4 d[NH3]/dt = -d[Cu(NH3)4]2+/dt
so for each trial the rate is = -1/4 d[NH3]/dt
for step 1 =0.030/428*4 = 1.75*10-5 mol l-1 sec-1
for step 2 =0.060/424*4 = 3.75*10-5 mol l-1 sec-1
for step 3 =0.030/210*4 =3.57*10-5 mol l-1 sec-1
for step 4 =0.030/35*4 =21.4*10-5 mol l-1 sec-1
2. answer: rate law expression = rate = K [Cu2+]0 [NH3]1
3. answer: Orderwith respect to Copper = from second and third trial on increasing concentrion from 0.010 M to 0.020 M rate remains constant so order is zero order
4. answer: Order with respect to ammonia = from first and second trial = on double the concentration , rate also double = [0.060]y/[0.030]y = 3.54*10-5/1.75*10-5
=[2]y =[2]1
so y = 1 means order is First Order
overall order = 0+1 = 1 (First Order)
6. answer: rate law constant = rate = K [Cu2+]0 [NH3]1
=[1.75*10-5] = K [0.010]0[0.030]1 =0.583*10-3 sec-1
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