1. Consider the reaction 2H3PO4P2O5+3H2O Using the information in the following
ID: 715185 • Letter: 1
Question
1. Consider the reaction
2H3PO4P2O5+3H2O
Using the information in the following table, calculate the average rate of formation of P2O5 between 10.0 and 40.0 s.
2. Consider the reaction
5Br(aq)+BrO3(aq)+6H+(aq)3Br2(aq)+3H2O(l)
The average rate of consumption of Br is 1.26×104M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval?
Express your answer with the appropriate units.
3. For a higher temperature, the curve would be For a higher temperature, the curve would be ______ spread out, the maximum of the curve would be _____ and to the ______ of the maximum of the red curve, and a _____ fraction of molecules would have kinetic energy greater than Ea than for the red curve.
Choices:
More, smaller, lower, right, left, greater, less, higher
Time (s) 0 10.0 20.0 30.0 40.0 50.0 [P2O5] (M) 0 1.70×103 4.70×103 6.50×103 7.70×103 8.30×103Explanation / Answer
1)
average rate of formation of P2O5 = change in concentration of P2O5 / change in time
= (C2-C1) / (t2-t1)
= (7.70*10^-3 - 1.70*10^-3) / (40.0-10.0)
= 6.00*10^-3 M / 30.0 s
= 2.00*10^-4 M/s
Answer: 2.00*10^-4 M/s
2)
Rate of reaction in terms of Br- is:
rate of reaction = (1/5)*rate of consumption of Br-
Rate of reaction in terms of Br2 is:
rate of reaction = (1/3)*rate of production of Br2
equate both rate of reaction:
(1/3)*rate of production of Br2 = (1/5)*rate of consumption of Br-
rate of production of Br2 = (3/5)*rate of consumption of Br-
= (3/5)*(1.26*10^-4 M/s)
= 7.56*10^-5 M/s
Answer: 7.56*10^-5 M/s
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