For the reaction A + 1/2 B --> 2 C, when C is increasing at a rate of 0.018 M/s, how fast is B decreasing?
To find how fast B is decreasing, we need to use the stoichiometry of the reaction.
Given that the reaction is: A + 1/2 B --> 2 C,
we can see that for every 1 mole of A consumed, 1/2 mole of B is consumed while 2 moles of C are produced.
So, we can write the rate of the reaction as:
rate = -Δ[A]/Δt = -(1/2) * Δ[B]/Δt = 2 * Δ[C]/Δt
Given that Δ[C]/Δt is 0.018 M/s, we can substitute this value into the equation:
0.018 M/s = 2 * Δ[C]/Δt
Now, solving for Δ[B]/Δt, we have:
Δ[B]/Δt = (0.018 M/s) / 2
Δ[B]/Δt = 0.009 M/s
Therefore, B is decreasing at a rate of 0.009 M/s.