The rate equation for the decomposition of N2O5 in CCl4 is, rate = K[N2O5], where K = 6.3 × 10-4 s–1 at 320 K. What would be the initial rate of decomposition of N2O5 in a 0.10 M solution of N2O5?

6 . 3 × 10 - 5 mol litre - 1 s - 1 , 0 . 63 × 10 - 4 mol litre s - 1 - 1

r = K · N 2 O 5 = 6 . 3 × 10 - 4 × ( 0 . 10 ) 1 = 6 . 3 × 10 - 5

0 . 63 × 10 - 6 mol litre - 1 s - 1

6 . 3 × 10 - 6 mol litre - 1 s - 1

6 . 3 × 10 - 5 mol litre - 1 s - 1

0 . 63 × 10 - 4 mol litre s - 1 - 1

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The rate equation for the decomposition of N₂O₅ in CCl₄ is, rate = K[N₂O₅], where K = 6.3 × 10^-4 s^–1 at 320 K. What would be the initial rate of decomposition of N₂O₅ in a 0.10 M solution of N₂O₅?

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$0.63 \times 10^{- 6} mol {litre}^{- 1} s^{- 1}$

$6.3 \times 10^{- 6} mol {litre}^{- 1} s^{- 1}$

$6.3 \times 10^{- 5} mol {litre}^{- 1} s^{- 1}$

$0.63 \times 10^{- 4} mol litre {{}^{- 1}s}^{- 1}$

answer is C, D.

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$r = K \cdot [N_{2} O_{5}] = 6.3 \times 10^{- 4} \times (0.10)^{1} = 6.3 \times 10^{- 5}$

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