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x + y + 2z → a + b
The following observations are made:
Tripling the initial concentration of X causes the rate of formation of A to be increased by a factor of 9.
Reducing the initial concentration of Y by 1/2 causes the rate of formation of A to be cut by 3/4.
Increasing the initial concentration of Z by 50% causes no change in the rate of formation of A.
Calculate the reaction order (solve for a, b, and c in the equation below) for X, Y, and Z based on the following empirical rate equation:
Rate = K[X]a[Y]b[Z]c
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