ClO3^-(aq)+3SO3^2- ¡÷ Cl^-(aq)+3SO4^2-
1) If the SO3^2- ion is disaapearing at rate of 0.458 mol/L*s, how fast is the Cl^- ion appearing?
2) if the after 10 minutes of reaction time, 1.09x10^-4 mole of Cl^- ion has been produced, how many moles of SO3^2- ion have been used up?
Please help I'm stuck with these 2 questions.
It works the same way as stoichiometry.
1.
0.458 x 1/3 = ?
2.
Same process as in #1.
@DrBob222 for number 2, is it 1.09x10^-4*1/3?
No, of course not.
#1. sulfite disappearance = 0.458 mol/L*s so
0.458 mol/L*s So3^2- x (1 mol Cl^-/3 mols So3^3-) = ?
So #2 must be what. Make those units cancel to come up with the unit you want.
1) To determine the rate at which the Cl^- ion is appearing, we need to use the stoichiometry of the balanced equation.
The balanced equation shows that for every 3 moles of SO3^2- consumed, 1 mole of Cl^- is produced. Therefore, the molar ratio is 1:3.
Given that the rate of disappearance of SO3^2- is 0.458 mol/L*s, we can calculate the rate of appearance of Cl^- as follows:
Rate of disappearance of SO3^2- = 0.458 mol/L*s
Rate of appearance of Cl^- = (0.458 mol/L*s) * (1 mol Cl^- / 3 mol SO3^2-)
Rate of appearance of Cl^- = 0.152 mol/L*s
Therefore, the Cl^- ion is appearing at a rate of 0.152 mol/L*s.
2) To determine the moles of SO3^2- ion used up after 10 minutes, we need to use the given information and the concept of reaction time.
First, we need to find the rate of appearance of Cl^- using the given data.
Rate of appearance of Cl^- = (1.09x10^-4 moles / 10 minutes) = (1.09x10^-5 moles/min)
Next, we can use the stoichiometric ratio to find the corresponding moles of SO3^2- used up for every mole of Cl^- produced.
From the balanced equation, we know that for every 3 moles of SO3^2- consumed, 1 mole of Cl^- is produced. Therefore, the molar ratio is 3:1.
So, the moles of SO3^2- used up can be calculated as follows:
Moles of SO3^2- = (1.09x10^-5 moles/min) * (3 moles SO3^2- / 1 mole Cl^-)
Moles of SO3^2- = 3.27x10^-5 moles/min
Therefore, after 10 minutes of reaction time, approximately 3.27x10^-5 moles of SO3^2- ion have been used up.