Welcome to the Quiz!
This quiz contains 7 questions from a mix of 1 subtopics.
The results above are obtained for the rate of reaction, A + B ➔ C.
What is the rate equation?
rate = k[A][B]2
rate = k[A][B]
rate = k[A]2[B]2
rate = k[A]2[B]
|
The rate equation for a reaction is rate = k[X]2[Y]. The initial rate of reaction is 5.4 x 10-4 mol dm-3 s-1 and the initial concentrations of X and Y are 0.010 mol dm-3 and 0.20 mol dm-3 respectively.
Calculate the value of k.
mol-2 dm6 s-1
|
What type of reaction produces the concentration-time graph shown above?
zero order
first order
second order
|
What type of reaction produces the rate-concentration graph shown above?
first order
second order
zero order
|
What type of reaction produces the rate-concentration graph shown above?
second order
first order
zero order
|
In an experiment, the concentration of iodide ions is varied, and the time taken for the solution to turn blue (t) is measured. The initial rate of reaction is equal to t1. The rate equation is given by rate = k[I-(aq)]. A graph of t1 against [I-(aq)] is plotted above.
Using the graph, calculate the value of the rate constant, k. Give your answer to 2 significant figures.
s-1
|
In an experiment, the concentration of iodide ions is varied, and the time taken for the solution to turn blue (t) is measured. The initial rate of reaction is equal to t1. The reaction is first order with respect to I-(aq).
Sketch the shape of the graph below.
|