For the reaction N2O5(g) $ \to $ 2NO2(g) + 1/2O2(g) the value of rate of disappearance of N2O5 is given as 6.25 $ \times $ 10$-$3 mol L$-$1 s$-$1. The rate of formation of NO2 and O2 is given respectively as

Question

For the reaction N₂O_5(g) $ \to $ 2NO_2(g) + 1/2O_2(g)
the value of rate of disappearance of N₂O₅ is given as 6.25 $ \times $ 10^$-$3 mol L^$-$1 s^$-$1. The rate of formation of NO₂ and O₂ is given respectively as

6.25 $ \times $ 10^$-$3 mol L^$-$1 s^$-$1 and
6.25 $ \times $ 10^$-$3 mol L^$-$1 s^$-$1

1.25 $ \times $ 10^$-$2 mol L^$-$1 s^$-$1 and
3.125 $ \times $ 10^$-$3 mol L^$-$1 s^$-$1

6.25 $ \times $ 10^$-$3 mol L^$-$1 s^$-$1 and
3.125 $ \times $ 10^$-$3 mol L^$-$1 s^$-$1

1.25 $ \times $ 10^$-$2 mol L^$-$1 s^$-$1 and
6.25 $ \times $ 10^$-$3 mol L^$-$1 s^$-$1

Solution

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