Given the following reaction: 5 Br-(aq) + BrO3-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l)

Question

If the rate of disappearance of bromate ions, BrO3-, is 1.45 mol/L·s, what is the corresponding rate of disappearance of hydrogen ions?

a) 0.24 mol/L·s
b) 0.29 mol/L·s
c) 0.48 mol/L·s
d) 2.9 mol/L·s
e) 7.3 mol/L·s

Answer 1

Looking at the balanced chemical equation:

5 Br-(aq) + BrO3-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l)

We can see that for every 6 moles of hydrogen ions (H+), we will produce 3 moles of bromate ions (BrO3-). Therefore, the rate of disappearance of hydrogen ions (H+) is half of the rate of disappearance of bromate ions (BrO3-).

Given that the rate of disappearance of bromate ions is 1.45 mol/L·s, the rate of disappearance of hydrogen ions will be half of that:

Rate of disappearance of hydrogen ions = 1.45 mol/L·s / 2 = 0.725 mol/L·s

Therefore, the corresponding rate of disappearance of hydrogen ions is approximately 0.725 mol/L·s, which is closest to option:

a) 0.24 mol/L·s

Answer 2

are you sure?

Answer 3

Apologies for the mistake. Let's recalculate the correct rate of disappearance of hydrogen ions (H+).

From the balanced chemical equation: 5 Br-(aq) + BrO3-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l)

We can see that for every 6 moles of hydrogen ions (H+), we will produce 3 moles of bromate ions (BrO3-). Therefore, the rate of disappearance of hydrogen ions (H+) is twice the rate of disappearance of bromate ions (BrO3-).

Given that the rate of disappearance of bromate ions is 1.45 mol/L·s, the rate of disappearance of hydrogen ions will be twice that:

Rate of disappearance of hydrogen ions = 1.45 mol/L·s x 2 = 2.9 mol/L·s

Therefore, the corresponding rate of disappearance of hydrogen ions is 2.9 mol/L·s, which is closest to option:

d) 2.9 mol/L·s.

Answer 4

what is the final and correct answer?

Answer 5

Apologies for the confusion. The correct answer is:

d) 2.9 mol/L·s