Answer:
Balancing the equation
2KMnO₂+10KCl+8H₂SO₄⇒2MnSO₄+6K₂SO₄+8H₂O+5Cl₂
Balance the reaction first:
3KOH + H3PO4 —> K3PO4 + 3H2O
So for every mol of H3PO4, you need 3 mol of OH- to fully neutralize the acid, since H3PO4 is polyprotic.
0.0200 L KOH • (2.000 mol KOH / L KOH) • (1 mol H3PO4 / 3 mol KOH) = 0.0133 mol H3PO4
Divide this by the volume of H3PO4 to get the concentration.
0.0133 mol H3PO4 / 0.0250 L = 0.532 M H3PO4
When it is summer in the Northern Hemisphere, it is winter in the Southern Hemisphere. It could be A I’m not sure if this helps.
<span>The object that was trying to be oxidized would end up being reduced. There would be no net reaction otherwise. The KCl would have simply melted after a long enough time and with the application of enough heat to the crucible.</span>
Use the Nernst equation which is:
E = E° - (RT/nF)*Ln Q
Where:
E the cell voltage in V,
R the gas constant 8.314 J/K•mol,
T the room temperature normally taken 298.15K, n=3 in this case,
F the Faraday constant 96485C,
Ln is the operation of natural logarithm, and: Q = [Cl-]^3*[Al3+]
Plugging in our values, will give us:
E = 1.88-(8.314*298.15/(3*96485))*Ln(0.010^3...)
= 2.01 (V)
