NO2 required for a reaction is produced by the decomposition of N2O5 in CCl4 as per the equation 2N2O5(g) arrow 4NO2(g) + O2(g). The initial concentration of N2O5 is 3.00 mol L-1 and it is 2.75 mol L-1 after 30 minutes. The rate of formation of NO2 is :

Question

NO2 required for a reaction is produced by the decomposition of N2O5 in CCl4 as per the equation 2N2O5(g) arrow 4NO2(g) + O2(g). The initial concentration of N2O5 is 3.00 mol L-1 and it is 2.75 mol L-1 after 30 minutes. The rate of formation of NO2 is : (A) 2.083 × 10-3 mol L-1 min-1 (B) 4.167 × 10-3 mol L-1 min-1 (C) 8.333 × 10-3 mol L-1 min-1 (D) 1.667 × 10-2 mol L-1 min-1

Tardigrade Admin · Accepted Answer

2N2 O5 (g) arrow 4NO2(g) + O2(g) 3.0 M 2.75 M (-Δ [N2O5]/Δ t) = (0.25/30) (1/2) ×(-Δ [N2O5]/Δ t) = (1/4) ×(- Δ [N2O5]/Δ t) = (1/4) ×(Δ [NO2]/Δ t) (Δ [NO2]/Δ t) = (0.25/30) ×2 = 1.66 ×10-2 M / min

$2.083 \times 1 0^{- 3} m o l L^{- 1} mi n^{- 1}$

$4.167 \times 1 0^{- 3} m o l L^{- 1} mi n^{- 1}$

$8.333 \times 1 0^{- 3} m o l L^{- 1} mi n^{- 1}$

$1.667 \times 1 0^{- 2} m o l L^{- 1} mi n^{- 1}$

Q. NO2​ required for a reaction is produced by the decomposition of N2​O5​ in CCl4​ as per the equation 2N2​O5​(g)→4NO2​(g)+O2​(g). The initial concentration of N2​O5​ is 3.00mol L−1 and it is 2.75mol L−1 after 30 minutes. The rate of formation of NO2​ is :

2.083×10−3molL−1min−1

4.167×10−3molL−1min−1

8.333×10−3molL−1min−1

1.667×10−2molL−1min−1

2N2​O5​(g)→4NO2​(g)+O2​(g) 3.0M 2.75 M Δt−Δ[N2​O5​]​=300.25​ 21​×Δt−Δ[N2​O5​]​=41​×Δt−Δ[N2​O5​]​=41​×ΔtΔ[NO2​]​ ΔtΔ[NO2​]​=300.25​×2=1.66×10−2M/min

$2.083 \times 1 0^{- 3} m o l L^{- 1} mi n^{- 1}$

$4.167 \times 1 0^{- 3} m o l L^{- 1} mi n^{- 1}$

$8.333 \times 1 0^{- 3} m o l L^{- 1} mi n^{- 1}$

$1.667 \times 1 0^{- 2} m o l L^{- 1} mi n^{- 1}$