The rate of formation of C in the reaction 2 A + B ----> 3 C + 2 D is 2.2 mol/L.s. Calculate the rates of reaction of A and B, and the rate of formation of D.
To determine the rates of reaction of A, B, and D, we need to relate them to the rate of formation of C.
In the given reaction, we are told that the rate of formation of C is 2.2 mol/L.s. This means that for every 3 moles of C formed, 2.2 moles of the reaction occurs per liter of the reaction mixture per second.
1. Calculating the rate of reaction of A:
Based on the stoichiometry of the reaction, we can see that for every 2 moles of A consumed, 3 moles of C are formed. Therefore, if the rate of formation of C is 2.2 mol/L.s, the rate of reaction of A can be calculated as follows:
rate of reaction of A = (2.2 mol/L.s) * (2 mol A / 3 mol C)
rate of reaction of A = 1.47 mol/L.s
So, the rate of reaction of A is 1.47 mol/L.s.
2. Calculating the rate of reaction of B:
Similarly, from the stoichiometry of the reaction, we know that for every 1 mole of B consumed, 3 moles of C are formed. Therefore, if the rate of formation of C is 2.2 mol/L.s, the rate of reaction of B can be calculated as follows:
rate of reaction of B = (2.2 mol/L.s) * (1 mol B / 3 mol C)
rate of reaction of B = 0.73 mol/L.s
Therefore, the rate of reaction of B is 0.73 mol/L.s.
3. Calculating the rate of formation of D:
Since D is a product of the reaction, its rate of formation is equal to the rate of consumption of A and B combined. This can be calculated as follows:
rate of formation of D = (2.2 mol/L.s) * (2 mol D / 3 mol C)
rate of formation of D = 1.47 mol/L.s
Hence, the rate of formation of D is 1.47 mol/L.s.
To summarize:
- Rate of reaction of A = 1.47 mol/L.s
- Rate of reaction of B = 0.73 mol/L.s
- Rate of formation of D = 1.47 mol/L.s