Question

For the reaction X + 2Y → P, the differential form equation of the rate law is:

• A. 2d[P]/dt = -d[Y]/dt
• B. -d[P]/dt = -d[X]/dt
• C. +d[X]/dt = -d[P]/dt
• D. -2d[Y]/dt = +d[P]/dt

Hint:

The coefficients in the rate law equation are often determined by the stoichiometry of the reaction. In this case, the change in concentration of Y is double that of P.

Answer 1

The Correct Option is A

For the reaction X + 2Y → P, the rate of change of concentration of P is twice that of Y, hence the rate law can be written as: \[ \frac{d[P]}{dt} = -\frac{d[Y]}{dt}/2 \] Thus, the correct equation is 2d[P]/dt = -d[Y]/dt.