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Tripling the initial concentration of x causes the rate of

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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Chemistry: Tripling the initial concentration of x causes the rate of

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