In a second experiment, which is performed at a much higher temperature, a sample of ethanol gas and a
copper catalyst are placed in a rigid, empty 1.0 L flask. The temperature of the flask is held constant, and the
initial concentration of the ethanol gas is 0.0100 M. The ethanol begins to decompose according to the
chemical reaction represented below. CH3CH2OH(g) æCuæà CH3CHO(g) + H2(g)
The concentration of ethanol gas over time is used to create the three graphs below.
(c) Given that the reaction order is zero, one, or two, use the information in the graphs to respond to the
following
(i) Determine the order of the reaction with respect to ethanol. Justify your answer.
The order of the reaction is zero. The plot on the left is a straight 1 point is earned for the correct
line, indicating that the rate of decrease in [ethanol] is constant as choice with a valid justification. [ethanol] changes. Therefore the rate of reaction does not depend
on [ethanol].
(ii) Write the rate law for the reaction
(iii) Determine the rate constant for the reaction, including units
(d) The pressure in the flask at the beginning of the experiment is 0.40 atm. If the ethanol completely
decomposes, what is the final pressure in the flask?