Textbook Question
(c) As a reaction proceeds, does the instantaneous reaction rate increase or decrease?
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Ch.14 - Chemical Kinetics
Chapter 14, Problem 19c
Consider the following hypothetical aqueous reaction: A(aq) → B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 (c) Between t = 10 min and t = 30 min, what is the average rate of appearance of B in units of M/s? Assume that the volume of the solution is constant.
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First, understand that the average rate of appearance of B is related to the rate of disappearance of A. Since the reaction is A → B, the rate of appearance of B is equal to the rate of disappearance of A.
Calculate the change in moles of A between t = 10 min and t = 30 min. This is done by subtracting the moles of A at 30 min from the moles of A at 10 min.
Determine the change in time in seconds between t = 10 min and t = 30 min. Since the time is given in minutes, convert this to seconds by multiplying the difference in minutes by 60.
Calculate the average rate of disappearance of A in moles per second by dividing the change in moles of A by the change in time in seconds.
Convert the rate from moles per second to molarity per second (M/s) by dividing the rate in moles per second by the volume of the solution in liters. Remember that 100.0 mL is equivalent to 0.100 L.
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Related Practice
Textbook Question
Consider the following hypothetical aqueous reaction: A(aq) → B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 (a) Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time zero and that A cleanly converts to B with no intermediates.
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Textbook Question
Consider the following hypothetical aqueous reaction: A(aq) → B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 (b) Calculate the average rate of disappearance of A for each 10-min interval in units of M>s.
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Textbook Question
A flask is charged with 0.100 mol of A and allowed to react to form B according to the hypothetical gas-phase reaction A1g2¡B1g2. The following data are collected: Time (s) 0 40 80 120 160 Moles of A 0.100 0.067 0.045 0.030 0.020 (c) Which of the following would be needed to calculate the rate in units of concentration per time: (i) the pressure of the gas at each time, (ii) the volume of the reaction flask, (iii) the temperature, or (iv) the molecular weight of A?
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Textbook Question
The isomerization of methyl isonitrile (CH3NC) to acetonitrile (CH3CN) was studied in the gas phase at 215°C, and the following data were obtained:
Time (s) [CH3NC] (M)
0 0.0165
2000 0.0110
5000 0.00591
8000 0.00314
12,000 0.00137
15,000 0.00074
(a) Calculate the average rate of reaction, in M/s, for the time interval between each measurement. (c) Which is greater, the average rate between t = 2000 and t = 12,000 s, or between t = 8000 and t = 15,000 s?
Textbook Question
The isomerization of methyl isonitrile (CH3NC) to acetonitrile (CH3CN) was studied in the gas phase at 215°C, and the following data were obtained:
Time (s) [CH3NC] (M)
0 0.0165
2000 0.0110
5000 0.00591
8000 0.00314
12,000 0.00137
15,000 0.00074
(b) Calculate the average rate of reaction over the entire time of the data from t = 0 to t = 15,000 s.
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