chemistry
posted by Alexis on .
Consider the reaction A + X products. Two trials are performed at the same temperature and using the same reaction medium. The initial rate is found to increase by a factor of 2.83 when the molar concentration of X is doubled and the molar concentration of A is unchanged.
(a) What is the order with respect to X?
(b) What can you determine about the order with respect to A from the information above?

rate 1 = 1 = k(X)^{a} where a is the order of the reaction.
rate 2 = 2.83 = k(2X)^{a}
Now take the ratio of equation 2 to equation 1 to obtain
2.83/1 = (2)^{a}
Solve for a which is the order of the reaction. I don't get a whole number. Check my thinking. Check my work.