Answer:
The balanced chemical equation for the reaction is:
2N₂O(g) → 4NO₂(g) + O₂(g)
To compare the rate of reaction of each component, we need to use the stoichiometry of the balanced equation to relate the rate of each component to the rate of O₂ production.
We know that 2.24 L of O₂ at NTP (0°C and 1 atm) are produced in 30 minutes. We can use the ideal gas law to convert this volume to moles:
n(O₂) = PV/RT = (1 atm)(2.24 L)/(0.08206 L atm/mol K)(273 K) = 0.102 mol
According to the balanced equation, 1 mole of O₂ is produced for every 2 moles of N₂O consumed. Therefore, the number of moles of N₂O consumed during the 30-minute reaction is:
n(N₂O) = 2 × n(O₂) = 2 × 0.102 mol = 0.204 mol
Similarly, the number of moles of NO₂ produced during the reaction is:
n(NO₂) = 4 × n(O₂) = 4 × 0.102 mol = 0.408 mol
Therefore, the rates of each component can be calculated as follows:
Rate of N₂O = n(N₂O) / t = 0.204 mol / 30 min = 0.0068 mol/min
Rate of NO₂ = n(NO₂) / t = 0.408 mol / 30 min = 0.0136 mol/min
Rate of O₂ = n(O₂) / t = 0.102 mol / 30 min = 0.0034 mol/min
Thus, the rate of NO₂ production is approximately twice the rate of N₂O consumption, and the rate of O₂ production is about half the rate of N₂O consumption.
I am not sure