The isomerization of methyl isonitrile (CH 3 NC) to acetonitrile (CH 3 CN) was studied in the gas phase at 215°C, and the following data were obtained: Time (s) [CH 3 NC] (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.

Hi everyone. This problem reads Rosane ion. I summarizes to an S. A. T assign ion at high temperatures for the given data. What is the average rate of the reaction from zero seconds to 10,000 seconds? Okay, so our goal here is to find find the average rate of the reaction and were given the time of zero seconds to 10, seconds. So let's just go ahead and highlight that here. So at zero seconds this is our concentration and at 10,000 seconds this is our concentration. Okay, so in order for us to find the average rate of the reaction, we're going to take our change in concentration over our change and time. Okay, So we're going to take our final minus our initial for both. And so we'll say this is our initial time and concentration and this is our final time and concentration. Okay, so our change in concentration is going to be final minus initial. So we have 0.023, -0.0293. That's our change in concentration over Our change in time. So our time is our final time is 10, seconds and our initial time is zero seconds. Alright, so this is what we're going to calculate and when we calculate that we're going to get an answer of 6. times 10 to the -7. This is going to be the average rate of reaction from zero seconds to 10,000 seconds four. This reaction. Okay, so that is it for this problem. I hope this was helpful

Ch.14 - Chemical Kinetics

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Brown 15th Edition

Ch.14 - Chemical Kinetics

Problem 21b

Chapter 14, Problem 21b

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.

Verified step by step guidance

Step 1: Identify the initial concentration of CH3NC at t = 0 s, which is 0.0165 M.

Step 2: Identify the final concentration of CH3NC at t = 15,000 s, which is 0.00074 M.

Step 3: Calculate the change in concentration of CH3NC over the time period, Δ[CH3NC] = [CH3NC]final - [CH3NC]initial.

Step 4: Calculate the total time interval, Δt = 15,000 s - 0 s.

Step 5: Use the formula for the average rate of reaction: Average rate = -Δ[CH3NC] / Δt.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Reaction Rate

The reaction rate is a measure of how quickly reactants are converted into products in a chemical reaction. It is typically expressed as the change in concentration of a reactant or product per unit time. In this case, the average rate can be calculated by determining the change in concentration of SCN- over the specified time interval.

Concentration Change

Concentration change refers to the difference in the concentration of a substance at two different times during a reaction. For the isomerization of methyl isonitrile to acetonitrile, the concentration of SCN- decreases over time, which is essential for calculating the average rate of reaction. This change is crucial for understanding how the reaction progresses.

Average Rate Calculation

The average rate of a reaction can be calculated using the formula: Average Rate = (Change in Concentration) / (Change in Time). For this problem, you would subtract the final concentration of SCN- from the initial concentration and divide by the total time elapsed. This provides a straightforward way to quantify the overall speed of the reaction over the given time period.

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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 (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.

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?

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

(d) Graph [CH₃NC] versus time and determine the instantaneous rates in M/s at t = 5000 s and t = 8000 s.

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Textbook Question

The rate of disappearance of HCl was measured for the following reaction: CH3OH1aq2 + HCl1aq2¡CH3Cl1aq2 + H2O1l2 The following data were collected: Time (min) 3HCl 4 1M2 0.0 1.85 54.0 1.58 107.0 1.36 215.0 1.02 430.0 0.580 (a) Calculate the average rate of reaction, in M>s, for the time interval between each measurement.

Textbook Question

The rate of disappearance of HCl was measured for the following reaction: CH3OH1aq2 + HCl1aq2¡CH3Cl1aq2 + H2O1l2 The following data were collected: Time (min) 3HCl 4 1M2 0.0 1.85 54.0 1.58 107.0 1.36 215.0 1.02 430.0 0.580 (b) Calculate the average rate of reaction for the entire time for the data from t = 0.0 min to t = 430.0 min.