In: Chemistry
The first column contains time in seconds and the second column the concentration of reactant in molar units.
e | 0.0256 |
0.1 | 0.0195 |
0.2 | 0.0143 |
0.3 | 0.0105 |
0.45 | 0.0074 |
0.5 | 0.0066 |
0.6 | 0.0060 |
0.7 | 0.0031 |
0.8 | 0.0024 |
0.9 | 0.0031 |
1 | 0.0019 |
1.1 | 0.0022 |
1.2 | 0.0005 |
1.3 | 0.0012 |
1.4 | 0.0006 |
1.5 | 0.0009 |
What is the rate constant of the reaction? Be sure you include units. Use "M" for molar and "s" for seconds ?
What is the rate of the reaction at t = 0.5s? Express your answer in units of M/s
What is the concentration of product at t = 0.5s?
We will plot graph between
a) concentration and time: If it is straight line then zero order reaction
b) ln[concentration] and time: if it is straight line then first order reaction
c) 1 / [concentration] and time: if it is straight line then second order reaction
The equation from graph is
y = -2.470x - 3.775
Rate constant = -slope = 2.470 s-1
b) rate of reaction = K[concentration] = 2.470 X [0.00660] = 0.0163 M/ s
c) concentration at t = 0.5 seconds = 0.00660 (as given)