Questions: This question has multiple parts. Work all the parts to get the most points. The reaction 2 NO(g)+2 H2(g) rightarrow N2(g)+2 H2O(g) was studied at 904^circC, and the data in the table were collected. Trial Reaction Concentration (mol/L) Rate of Appearance of N (mol/L-s) --------- [NO] [H2] 1 0.420 0.122 0.136 2 0.210 0.122 0.0339 3 0.210 0.244 0.0678 4 0.105 0.488 0.0339 Which two reaction trials can be used to determine the order of the reaction in [NO]? and

Solution Steps

The reaction given is: \[ 2 \mathrm{NO}(g) + 2 \mathrm{H}_{2}(g) \rightarrow \mathrm{N}_{2}(g) + 2 \mathrm{H}_{2} \mathrm{O}(g) \]

The rate of appearance of \(\mathrm{N}_{2}\) is provided for different trials with varying concentrations of \([\mathrm{NO}]\) and \([\mathrm{H}_{2}]\).

To determine the order of the reaction with respect to \([\mathrm{NO}]\), we need to compare trials where the concentration of \([\mathrm{H}_{2}]\) remains constant while \([\mathrm{NO}]\) changes. This allows us to isolate the effect of \([\mathrm{NO}]\) on the reaction rate.

From the data:

• Trials 1 and 2 have the same \([\mathrm{H}_{2}]\) concentration of 0.122 mol/L, but different \([\mathrm{NO}]\) concentrations (0.420 mol/L and 0.210 mol/L, respectively).

These trials can be used to determine the order of the reaction with respect to \([\mathrm{NO}]\).

Final Answer