Given the following reaction: 5 Br-(aq) + BrO3-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l)
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
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
are you sure?
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.
what is the final and correct answer?
Apologies for the confusion. The correct answer is:
d) 2.9 mol/L·s
To find the corresponding rate of disappearance of hydrogen ions (H+), we need to use the balanced chemical equation and the stoichiometric coefficients.
The balanced chemical equation is:
5 Br-(aq) + BrO3-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l)
By looking at the coefficients, we can see that the ratio of H+ to BrO3- is 6:1. This means that for every 6 moles of H+ consumed, 1 mole of BrO3- is consumed.
Since the rate of disappearance of BrO3- is given as 1.45 mol/L·s, we can use this information to find the rate of disappearance of H+. We multiply the rate of disappearance of BrO3- by the stoichiometric coefficient ratio:
Rate of disappearance of H+ = (1.45 mol/L·s) * (6 mol H+/1 mol BrO3-) = 8.7 mol/L·s
Therefore, the corresponding rate of disappearance of hydrogen ions is 8.7 mol/L·s.
None of the answer choices given match this value. It's possible that there may be an error in the provided answer choices, or the question may need to be reevaluated.