For the reaction shown below, the instantaneous rate of formation of Br(aq) is 0.12 M/s at t=2.0 min.
3Br0(aq) -> BrO3(aq) + 2Br(aq)
What are the instantaneous rates of formation of BrO3(aq) and consumption of BrO(aq)?
To determine the instantaneous rates of formation of BrO3(aq) and consumption of BrO(aq), we can use the stoichiometric coefficients of the balanced chemical equation.
The chemical equation is:
3BrO(aq) -> BrO3(aq) + 2Br(aq)
The coefficients in the balanced equation tell us the stoichiometric relationship between the reactants and products. In this case, the coefficient of BrO3(aq) is 1, while the coefficient of BrO(aq) is -3 (because it is being consumed).
Given that the instantaneous rate of formation of Br(aq) is 0.12 M/s at t=2.0 min, we can use this information to determine the instantaneous rates of formation of BrO3(aq) and consumption of BrO(aq).
First, let's use the rate of formation of Br(aq) to find the rate of formation of BrO3(aq):
Since the coefficient of Br in the balanced equation is 2, the rate of formation of BrO3(aq) is also 2 times the rate of formation of Br(aq).
Rate of formation of BrO3(aq) = 2 * 0.12 M/s = 0.24 M/s
Next, let's use the rate of formation of Br(aq) to find the rate of consumption of BrO(aq):
Since the coefficient of BrO(aq) in the balanced equation is -1/3 (or -1 for simplicity), the rate of consumption of BrO(aq) is equal to the rate of formation of Br(aq).
Rate of consumption of BrO(aq) = 0.12 M/s
Therefore, the instantaneous rate of formation of BrO3(aq) is 0.24 M/s, and the instantaneous rate of consumption of BrO(aq) is 0.12 M/s.