Chemical Kinetics
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4.2 In a reaction, 2A → Products, the concentration of A decreases from 0.5 mol L–1 to 0.4 mol L–1 in 10 minutes. Calculate the rate during this interval?
4.2 In a reaction, 2A → Products, the concentration of A decreases from 0.5 mol L–1 to 0.4 mol L–1 in 10 minutes. Calculate the rate during this interval?
4.2 Given-
Initial concentration (A1) = 0.5M
Final concentration (A2) = 0.4M
Time = 10 mins.
The formula for average rate of the reaction is,
rav = -1/2 X Δ{A} / Δt → Equation 1
? {A} = (A2)-( A1), the equation 1 is written as,
rav = -1/2 X A2 - A1 / Δt
= -1/2 X 0.4-0.5 / 10
= -1/2 X 0.1 / 10
= 0.00
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4.1 For the reaction R → P, the concentration of a reactant changes from 0.03M to 0.02M in 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.
4.1 For the reaction R → P, the concentration of a reactant changes from 0.03M to 0.02M in 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.
4.1 Given-
Initial concentration (R1) = 0.03M
Final concentration (R2) = 0.02M
Time = 25 mins.
The formula for average rate of the reaction is,
rav = - Δ{R} / Δt → Equation 1
? {R} = (R2)-( R1), the equation 1 is written as,
rav = - R2 - R1 / Δt
= -0.02-0.03 / 25
= 4 X 10-4 mol L-1 min-1
The average rate of r
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