This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Here's how to calculate the rates based on the given data and balanced equation 2X + 4Y → 3Z + 5Q. The initial data for Y is: [Y]_initial = 1.350 M at t_initial = 0.00 s [Y]_final = 0.407 M at t_final = 11.9 s Step 1: Calculate the rate of disappearance of Y. The rate of disappearance of Y is given by the negative change in concentration of Y over the change in time. -([Y])/( t) = -([Y]_final - [Y]_initial)(t_final - t_initial) -([Y])/( t) = -(0.407 M - 1.350 M)(11.9 s - 0.00 s) -([Y])/( t) = -(-0.943 M)11.9 s -([Y])/( t) = 0.079243697 M/s Rounding to three significant figures: a) The rate of disappearance of Y: 0.0792 M/s Step 2: Calculate the rates of disappearance of X and appearance of Z and Q using stoichiometry. The general relationship between rates for the reaction 2X + 4Y → 3Z + 5Q is: Rate = -(1)/(2)([X])/( t) = -(1)/(4)([Y])/( t) = (1)/(3)([Z])/( t) = (1)/(5)([Q])/( t) b) The rate of disappearance of X: -([X])/( t) = (2)/(4) × (-([Y])/( t)) -([X])/( t) = (1)/(2) × 0.079243697 M/s -([X])/( t) = 0.0396218485 M/s Rounding to three significant figures: 0.0396 M/s c) The rate of appearing of Z: ([Z])/( t) = (3)/(4) × (-([Y])/( t)) ([Z])/( t) = (3)/(4) × 0.079243697 M/s ([Z])/( t) = 0.05943277275 M/s Rounding to three significant figures: 0.0594 M/s d) The rate of appearing of Q: ([Q])/( t) = (5)/(4) × (-([Y])/( t)) ([Q])/( t) = (5)/(4) × 0.079243697 M/s ([Q])/( t) = 0.09905462125 M/s Rounding to three significant figures: 0.0991 M/s e) The overall rate of reaction: The overall rate of reaction can be calculated using any species, divided by its stoichiometric coefficient. Using Y: Overall Rate = -(1)/(4)([Y])/( t) Overall Rate = (1)/(4) × 0.079243697 M/s Overall Rate = 0.01981092425 M/s Rounding to three significant figures: 0.0198 M/s Send me the next one 📸