Question

for the reaction 2 a 4 b → 2 c 4 d, what is the absolute magnitude of the rate of change for [b] when [c] is increasing at 2.0 m/s?

Answer 1

The absolute rate of change for [B] when [C] is increasing at a rate of 2.0 M/s is 4.0 M/s, due to the stoichiometric relationship in the reaction 2 A + 4 B → 2 C + 4 D.

Step-by-step explanation:

For the chemical reaction 2 A + 4 B → 2 C + 4 D, when the concentration of [C] increases at a rate of 2.0 M/s, we want to find the rate of change of [B]. To find this, we look at the stoichiometry of the reaction. The reaction shows that for every 2 moles of C produced, 4 moles of B are consumed. Therefore, the rate at which B is consumed is twice the rate at which C is formed.

Since [C] is increasing at 2.0 M/s, the rate of change for [B] (the rate at which B is consumed) would be 2 times 2.0 M/s, which equals 4.0 M/s. Remember, we take the absolute value of this rate because rates of reaction are typically expressed as positive values, indicating the rate of production for products or the rate of consumption for reactants.