The experimental data for decomposition of N2O5 [2N2O5→4NO2+O2] in g

1.	The experimental data for decomposition of N2O5 [2N2O5→4NO2+O2] in gas phase at 318 K are given below: t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Plot [N2O5] against t t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Find the half-life period for the reaction t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Draw a graph between log[N2O5] and t t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 What is the rate law? t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Calculate the rate constant t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Calculate the half-life period from k and compare it with (ii)
Answer» The experimental data for decomposition of $N_{2} O_{5}$ $[2 N_{2} O_{5} \to 4 N O_{2} + O_{2}]$ in gas phase at 318 K are given below: $\begin{matrix} t / s & 0 & 400 & 800 & 1200 & 1600 & 2000 & 2400 & 2800 & 3200 10^{- 2} \times [N_{2} O_{5}] / & 1.63 & 1.36 & 1.14 & 0.93 & 0.78 & 0.64 & 0.53 & 0.43 & 0.35 m o l L^{- 1} \end{matrix}$ Plot $[N_{2} O_{5}]$ against t $\begin{matrix} t / s & 0 & 400 & 800 & 1200 & 1600 & 2000 & 2400 & 2800 & 3200 10^{- 2} \times [N_{2} O_{5}] / & 1.63 & 1.36 & 1.14 & 0.93 & 0.78 & 0.64 & 0.53 & 0.43 & 0.35 m o l L^{- 1} \end{matrix}$ Find the half-life period for the reaction $\begin{matrix} t / s & 0 & 400 & 800 & 1200 & 1600 & 2000 & 2400 & 2800 & 3200 10^{- 2} \times [N_{2} O_{5}] / & 1.63 & 1.36 & 1.14 & 0.93 & 0.78 & 0.64 & 0.53 & 0.43 & 0.35 m o l L^{- 1} \end{matrix}$ Draw a graph between $l o g [N_{2} O_{5}]$ and t $\begin{matrix} t / s & 0 & 400 & 800 & 1200 & 1600 & 2000 & 2400 & 2800 & 3200 10^{- 2} \times [N_{2} O_{5}] / & 1.63 & 1.36 & 1.14 & 0.93 & 0.78 & 0.64 & 0.53 & 0.43 & 0.35 m o l L^{- 1} \end{matrix}$ What is the rate law? $\begin{matrix} t / s & 0 & 400 & 800 & 1200 & 1600 & 2000 & 2400 & 2800 & 3200 10^{- 2} \times [N_{2} O_{5}] / & 1.63 & 1.36 & 1.14 & 0.93 & 0.78 & 0.64 & 0.53 & 0.43 & 0.35 m o l L^{- 1} \end{matrix}$ Calculate the rate constant $\begin{matrix} t / s & 0 & 400 & 800 & 1200 & 1600 & 2000 & 2400 & 2800 & 3200 10^{- 2} \times [N_{2} O_{5}] / & 1.63 & 1.36 & 1.14 & 0.93 & 0.78 & 0.64 & 0.53 & 0.43 & 0.35 m o l L^{- 1} \end{matrix}$ Calculate the half-life period from k and compare it with (ii)

The experimental data for decomposition of N2O5 [2N2O5→4NO2+O2] in gas phase at 318 K are given below: t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Plot [N2O5] against t t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Find the half-life period for the reaction t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Draw a graph between log[N2O5] and t t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 What is the rate law? t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Calculate the rate constant t/s040080012001600200024002800320010−2×[N2O5]/1.631.361.140.930.780.640.530.430.35mol L−1 Calculate the half-life period from k and compare it with (ii)

Answer»

The experimental data for decomposition of $N_{2} O_{5}$ $[2 N_{2} O_{5} \to 4 N O_{2} + O_{2}]$ in gas phase at 318 K are given below:

$\begin{matrix} t / s & 0 & 400 & 800 & 1200 & 1600 & 2000 & 2400 & 2800 & 3200 10^{- 2} \times [N_{2} O_{5}] / & 1.63 & 1.36 & 1.14 & 0.93 & 0.78 & 0.64 & 0.53 & 0.43 & 0.35 m o l L^{- 1} \end{matrix}$

Plot $[N_{2} O_{5}]$ against t

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