Under certain conditions, the reaction
3A + 2B -> 4C
was observed to proceed at a rate of
0.00348 M· s−1. What was the corresponding
rate of change in reactant A?
Well, let's see here. According to the balanced chemical equation, for every 3 moles of A that react, 4 moles of C are produced. So, if the reaction rate is 0.00348 M·s−1, we can assume that for every second that passes, 0.00348 moles of C are produced.
Since the stoichiometry tells us that 3 moles of A react to produce 4 moles of C, we can use this ratio to find the corresponding rate of change in reactant A.
So, for every 4 moles of C produced, we'll need 3 moles of A to react. Therefore, the rate of change in reactant A is (0.00348 M·s−1) x (3 moles A / 4 moles C).
But since we want the rate in terms of A, we'll divide this by the molar coefficient of A in the balanced equation, which is 3.
So, the corresponding rate of change in reactant A would be (0.00348 M·s−1) x (3 moles A / 4 moles C) / 3 = 0.00261 M·s−1.
Whew, that was a lot of math! Hope I didn't clown around too much.
To determine the rate of change in reactant A, we need to use the stoichiometric coefficients of A and C in the balanced chemical equation.
The balanced chemical equation is:
3A + 2B -> 4C
From the balanced equation, we can see that the stoichiometric coefficient of A is 3, meaning that for every 3 moles of A reacted, 4 moles of C are produced.
The rate of change in reactant A can be calculated using the following formula:
Rate of change in reactant A = -(1/stoichiometric coefficient of A) * (rate of reaction)
In this case, the stoichiometric coefficient of A is 3.
Rate of change in reactant A = -(1/3) * (0.00348 M· s−1)
Rate of change in reactant A = -0.00116 M· s−1
Therefore, the corresponding rate of change in reactant A is -0.00116 M· s−1.
To determine the rate of change in reactant A, we need to consider the stoichiometry of the reaction. The stoichiometry tells us the ratio of the reactants and products involved in the reaction.
According to the given reaction: 3A + 2B -> 4C, the stoichiometric coefficients for reactant A and product C are 3 and 4 respectively.
The rate of change for reactant A can be related to the rate of the reaction by the formula:
Rate of Change of Reactant A = -(1/3) * (rate of reaction)
This is because for every 3 moles of reactant A consumed, 4 moles of product C are formed. Therefore, the negative sign is included to account for the decreasing concentration of reactant A.
Now, we can calculate the rate of change in reactant A using the given rate of reaction:
Rate of Change of Reactant A = -(1/3) * (0.00348 M·s−1)
= -0.00116 M·s−1
Therefore, the corresponding rate of change in reactant A is -0.00116 M·s−1.
rate = -(1/3)(change in A)/time.
0.00348 = -(1/3)dA/dt.
Solve for dA/dT