For the reaction: N_2O_5(g) rightarrow 2NO_2(g) + 1/2O_2(g) If N_2O_5 is decompo

Question

For the reaction: N_2O_5(g) rightarrow 2NO_2(g) + 1/2O_2(g) If N_2O_5 is decomposing with an instantaneous rate of 4.43 mol/L-5, what is the instantaneous rate of formation of NO_2? For the reaction: N_2O_5(g) rightarrow 2NO_2(g) + 1/2O_2(g), If the concentration of N_2O_5 drops from 1.5 mol/L drops to 0.18 mol/L in a one L flask, how many grams of O_2 been have formed? For the reaction: A(g) rightarrow B(g). the rate of disappearance of A is directly proportional to the concentration of A. If the instantaneous rate for the disappearance of A is 5.29 mol/L-5 at 0.91 mol/L what is the rate constant, k, for this reaction?

Explanation / Answer

1. From the given equation we can infer that

Rate of decomposition of N2O5= (rate of formation of NO2)÷2

given rate of decomposition of N2O5=4.43 mol/ls

so rate of formation of NO2:- 2×4.43=8.86M/s

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