Answer: The lead-containing reactant(s) consumed during recharging of a lead-acid battery is
Explanation:
In lead acid battery, the anode is made up of lead and undergoes oxidation during discharging and cathode is made up of lead oxide and acts as cathode during discharging. The electrolyte used is dilute .
Charging:
Cathode : reduction :
Anode: oxidation :
Overall reaction :
The lead-containing reactant(s) consumed during recharging of a lead-acid battery is
Answer:
a) Number-average molar mass: 163,700g/mol
Weight-average molar mass: 200,000g/mol
b) Number-average molar mass: 200,000g/mol
Weight-average molar mass: 233,300g/mol
Explanation:
The number-average molar mass is based on mole% and weight-average molar mass is based on weight%, thus:
a) In equal proportions by weight:
number-average molar mass:
1g A× = 1x10⁻⁵ moles A
1g B× = 5x10⁻⁶ moles B
1g C× = 3,33x10⁻⁶ moles C
Total moles are:
1x10⁻⁵ A + 5x10⁻⁶ B + 3,33x10⁻⁶ C = 1,833x10⁻⁵ moles.
Percent A: ×100 = 54,5%
Percent B: ×100 = 27,3%
Percent C: ×100 = 18,2%
number-average molar mass:
0,545*100,000g/mol + 0,273*200,000g/mol + 0,182*300,000g/mol = 163,700g/mol
weight-average molar mass:
0,333*100,000g/mol + 0,333*200,000g/mol + 0,333*300,000g/mol = 200,000g/mol
b) In molar ratio 1:1:1
weight-average molar mass:
1mol A× = 100,000g A
1mol B× = 200,000g B
1mol C× = 300,000g C
Total mass is:
100,000 A + 200,000 B + 300,000 C = 600,000 g.
Percent A: ×100 = 16,7%
Percent B: ×100 = 33,3%
Percent C: ×100 = 50,0%
Weight-average molar mass:
0,167*100,000g/mol + 0,333*200,000g/mol + 0,500*300,000g/mol = 233,300g/mol
number-average molar mass:
0,333*100,000g/mol + 0,333*200,000g/mol + 0,333*300,000g/mol = 200,000g/mol
I hope it helps!