I will assume the chemical reaction equation is like this:
<span>Ba(NO3)2 + Na2SO4 ---> 2 NaNO3 + BaSO4
</span>
For every 1 barium nitrate molecule used, there will be 1 barium sulfate formed. The number of molecule barium sulfate formed would be: <span>20.00 ml * 0.500 mol/1000ml * 1= 0.01 mol
The mass of barium sulfate produced: 0.01mol * </span>233.38 g/mol= 2.3338 grams
The corresponding value that is the least precise would be A. As it only contains 1 value that is a significant digit, 1.
Answer:
Mn^2+(aq) + 4H2O(l) + 5[VO2]^+(aq) + 10H^+(aq) ---------->MnO4^-(aq) + 8H^+(aq) + 5[VO]^2+(aq) + 5H2O(l)
Explanation:
Oxidation half equation:
Mn^2+(aq) + 4H2O(l) ------------> MnO4^-(aq) + 8H^+(aq) + 5e
Reduction half equation:
5[VO2]^+(aq) + 10H^+(aq) + 5e --------> 5[VO]^2+(aq) + 5H2O(l)
Overall redox reaction equation:
Mn^2+(aq) + 4H2O(l) + 5[VO2]^+(aq) + 10H^+(aq) ---------->MnO4^-(aq) + 8H^+(aq) + 5[VO]^2+(aq) + 5H2O(l)
