What is the activation energy for the decomposition of N2O5 as N2O5g⇌ 2NO2g+12O2g if the values of the rate constants are 3.45×10-5 and 6.9 ×10-3 at 27°C and 67°C respectively

Decomposition of N2O5 isN2O5⇌2NO2+O2log K2K1=Ea2.303 R1T1-1T2log 6.9×10-33.55×10-5=Ea8.314×2.303 40300×340log 2×102=Ea×402.3×8.314×2.303×300×340 Ea=11200J =112 KJ

What is the activation energy for the decomposition of N2O5 as N2O5g⇌ 2NO2g+12O2g if the values of the rate constants are 3.45×10-5 and 6.9 ×10-3 at 27°C and 67°C respectively

Decomposition of N2O5 isN2O5⇌2NO2+O2log K2K1=Ea2.303 R1T1-1T2log 6.9×10-33.55×10-5=Ea8.314×2.303 40300×340log 2×102=Ea×402.3×8.314×2.303×300×340 Ea=11200J =112 KJ

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What is the activation energy for the decomposition of $N_{2} O_{5} as N_{2} O_{5 (g)} ⇌ 2 {NO}_{2 (g)} + \frac{1}{2} O_{2 (g)}$ if the values of the rate constants are $3.45 \times 10^{- 5} and 6.9 \times 10^{- 3} at 27 ° C and 67 ° C respectively$

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$102 \times 10^{2} KJ$

488.5 kJ

112 kJ

224 kJ

answer is C.

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Detailed Solution

Decomposition of $N_{2} O_{5} is$

$N_{2} O_{5} ⇌ 2 {NO}_{2} + O_{2}$

$\log \frac{K_{2}}{K_{1}} = \frac{E_{a}}{2.303 R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$

$\log [\frac{6.9 \times 10^{- 3}}{3.55 \times 10^{- 5}}] = \frac{E_{a}}{8.314 \times 2.303} [\frac{40}{300 \times 340}]$ $\log [2 \times 10^{2}] = \frac{E_{a} \times 40}{2.3 \times 8.314 \times 2.303 \times 300 \times 340}$ $E_{a} = 11200 J = 112 KJ$