A student conducted an experiment to determine what factors are important in the rate of reaction between potassium carbonate and hydrochloric acid. The student diluted 4.000 mL of 4.000 M K2CO3 to 150.0 mL, then combined that solution with 150.00 mL of 2.000 M HCl at an increased temperature of 50 °C.
The student tabulated the amount of CO2 gas collected over time and recorded the results in the columns to the left.
1. Use a rearrangement of PV = nRT to solve for the number of moles of CO2 produced. You may assume atmospheric pressure. Enter (and fill down) your formula in column C.
Need help on equation to solve for C.
Time (min) |
Volume (mL) |
|
1 |
3.7 |
|
2 |
7.5 |
|
3 |
11.2 |
|
4 |
15 |
|
5 |
18.7 |
|
6 |
22.5 |
|
7 |
26.2 |
|
8 |
30 |
|
9 |
33.7 |
|
10 |
37.5 |
|
11 |
41.2 |
|
12 |
45 |
|
13 |
48.7 |
|
14 |
52.5 |
|
15 |
56.2 |
|
16 |
60 |
|
17 |
63.7 |
|
18 |
67.5 |
|
19 |
71.2 |
|
20 |
75 |
A student conducted an experiment to determine what factors are important in the rate of reaction...