The table to the right gives the concentrations of C2H4O(g) as a function of time at a certain t

For this question, it simply wants us to verify that this is a first -order reaction. To do that

In answering this question, we have to first of all look into the chemical equation of what is a

The reaction in this problem shows the decomposition of ethylene oxide forming methane and carbo

So let's say we've got a reaction in which we've got A that is being consumed to form product B.

To correctly answer this equation, the best way is to use Excel and plot the data. You need to p

Question

The table to the right gives the concentrations of \( \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}(\mathrm{g}) \) as a function of time at a certain temperature for the following reaction \[ \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}(\mathrm{~g}) \rightarrow \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{CO}(\mathrm{~g}) \] Find the order of this reaction and the value of the rate constant. \begin{tabular}{|c|c|} \hline\( \left[\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\right](\mathrm{M}) \) & time \( (\mathbf{m i n}) \) \\ \hline 0.0860 & 0.00 \\ \hline 0.0465 & 50.0 \\ \hline 0.0355 & 72.0 \\ \hline 0.0274 & 93.0 \\ \hline 0.0174 & 130.0 \\ \hline \end{tabular} Order of the reaction. First Order Zeroth Order Second Order value of the rate constant: \( \square \)

          The table to the right gives the concentrations of \( \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}(\mathrm{g}) \) as a function of time at a certain temperature for the following reaction
\[
\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}(\mathrm{~g}) \rightarrow \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{CO}(\mathrm{~g})
\]

Find the order of this reaction and the value of the rate constant.
\begin{tabular}{|c|c|}
\hline\( \left[\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\right](\mathrm{M}) \) & time \( (\mathbf{m i n}) \) \\
\hline 0.0860 & 0.00 \\
\hline 0.0465 & 50.0 \\
\hline 0.0355 & 72.0 \\
\hline 0.0274 & 93.0 \\
\hline 0.0174 & 130.0 \\
\hline
\end{tabular}

Order of the reaction.
First Order
Zeroth Order
Second Order
value of the rate constant:
\( \square \)

The table to the right gives the concentrations of C2H4O(g) as a function of time at a certain temperature for the following reaction

C2H4O( g) →CH4( g)+CO( g)

Find the order of this reaction and the value of the rate constant.

[C2H4O](M) time (𝐦 𝐢 𝐧)

0.0860 0.00

0.0465 50.0

0.0355 72.0

0.0274 93.0

0.0174 130.0

Order of the reaction.
First Order
Zeroth Order
Second Order
value of the rate constant:
□

Added by Julian H.

Question

Please give Ace some feedback