The partial pressures of the gases in the container are monitored at constant temperature and recorded in the table below. At time t4, is the rate of the reverse reaction greater than, less than, or equal to the rate of the forward reaction? At equilibrium, the container holds fewer molecules of which gas, Cl2(g) or O2(g) ?
time - PCl2 (atm) - PO2 (atm) - PCl2O (atm)
t0 - 0.50 - 0.50 - 0.0
t1 - 0.42 - 0.46 - 0.08
t2 - 0.36 - 0.43 - 0.14
t3 - 0.32 - 0.41 - 0.19
t4 - 0.29 - 0.39 - 0.22
t5 - 0.27 - 0.38 - 0.23
t6 - 0.26 - 0.37 - 0.24
t7 - 0.25 - 0.38 - 0.25
t8 - 0.25 - 0.38 - 0.25
t9 - 0.25 - 0.38 - 0.25
I assume the time intervals are the same; i.e., 1 sec or 2 sec or 3 sec etc.
rate of the rxn = delta pO2/delta time = ?
Follow O2 down the chart.
rate from t = 0 to t = 1 is 0.04
t1 to t2 = 0.03
t2 to t3 = 0.02
t3 to t4 = 0.02
t4 to t5 = 0.01
Since the rate of the forward reaction from t3 to t4 and from t4 to t5 is positive, then the forward reaction is faster than the reverse so the reverse reaction is less than the forward reaction.
For the gas with the fewest molecules, I would do the following.
From t9 that looks like equilibrium so lowest pressure has fewest moles and fewest moles will have fewest molecules. Which has the fewest moles?
ed
At time t4, the rate of the reverse reaction is greater than the rate of the forward reaction because the partial pressure of PCl2 is decreasing while the partial pressure of PCl2O is increasing.
At equilibrium, the container holds fewer molecules of Cl2(g) because the partial pressure of Cl2(g) is decreasing while the partial pressure of PCl2O is increasing. So, Cl2(g) is being consumed while PCl2O is being formed. It seems like Cl2(g) is the popular one at the party!
To determine if the rate of the reverse reaction is greater than, less than, or equal to the rate of the forward reaction at time t4, we can compare the changes in the partial pressures of the gases over time.
From the table, we can see that the partial pressure of Cl2 decreases from t0 to t4, indicating that the forward reaction is occurring. On the other hand, the partial pressure of PCl2O increases from t0 to t4, indicating that the reverse reaction is occurring.
To determine if the rate of the reverse reaction is greater than, less than, or equal to the rate of the forward reaction at time t4, we can compare the changes in the partial pressures of the gases from t3 to t4.
From t3 to t4, the partial pressure of Cl2 decreases by 0.03 atm, while the partial pressure of PCl2O increases by 0.03 atm. This tells us that the rate of the reverse reaction is equal to the rate of the forward reaction at time t4.
At equilibrium, the container holds fewer molecules of Cl2(g) compared to O2(g). This can be determined by comparing the initial and final partial pressures of Cl2 and O2.
From the table, at t0, the partial pressure of Cl2 is 0.50 atm, while the partial pressure of O2 is also 0.50 atm. However, at equilibrium (t9), the partial pressure of Cl2 is 0.25 atm, while the partial pressure of O2 remains at 0.38 atm. Therefore, at equilibrium, the container holds fewer molecules of Cl2(g) than O2(g).
To determine if the rate of the reverse reaction is greater than, less than, or equal to the rate of the forward reaction at time t4, we need to compare the changes in partial pressures of the reactants and products.
At t4, the partial pressure of PCl2 is 0.29 atm, and the partial pressure of PO2 is 0.39 atm.
To find the rate of the forward reaction, we can compare the changes in partial pressures of the reactants. From t0 to t4, the partial pressure of PCl2 decreased from 0.50 atm to 0.29 atm, which is a decrease of 0.21 atm.
To find the rate of the reverse reaction, we compare the changes in partial pressures of the products. From t0 to t4, the partial pressure of PCl2O increased from 0.0 atm to 0.22 atm, which is an increase of 0.22 atm.
Comparing the changes, we see that the decrease in the partial pressure of PCl2 (0.21 atm) is greater than the increase in the partial pressure of PCl2O (0.22 atm). Therefore, at time t4, the rate of the forward reaction is greater than the rate of the reverse reaction.
To determine which gas has fewer molecules at equilibrium, we need to compare the equilibrium partial pressures of Cl2(g) and O2(g). At equilibrium, the partial pressure of Cl2(g) is 0.25 atm, while the partial pressure of O2(g) is 0.38 atm.
Since the number of molecules is directly proportional to the partial pressure, the gas with the lower partial pressure has fewer molecules. Therefore, at equilibrium, the container holds fewer molecules of Cl2(g) than O2(g).