Answer:
3.81 g Pb
Explanation:
When a lead acid car battery is recharged, the following half-reactions take place:
Cathode: PbSO₄(s) + H⁺ (aq) + 2e⁻ → Pb(s) + HSO₄⁻(aq)
Anode: PbSO₄(s) + 2 H₂O(l) → PbO₂(s) + HSO₄⁻(aq) + 3H⁺ (aq) + 2e⁻
We can establish the following relations:
- 1 A = 1 c/s
- 1 mole of Pb(s) is deposited when 2 moles of e⁻ circulate.
- The molar mass of Pb is 207.2 g/mol
- 1 mol of e⁻ has a charge of 96468 c (Faraday's constant)
Suppose a current of 96.0A is fed into a car battery for 37.0 seconds. The mass of lead deposited is:
Answer:
For eacht 4 moles Fe consumed, we will produce 2 moles Fe2O3
The mole ration is 4:2 (option 1)
Explanation:
Step 1: The unbalanced equation
Fe + O2 → Fe2O3
Step 2: Balancing the equation
Fe + O2 → Fe2O3
On the left side we have 2x O (in O2) and on the right side we have 3x O (in Fe2O3) . To balance the amount of O on both sides, we have to multiply O2 by 3 and Fe2O3 by 2.
Fe + 3O2 → 2Fe2O3
On the left side we have 1x Fe, On the right side we have 4x (in 2Fe2O3). To balance the amount of Fe we have to multiply Fe (on the left side) by 4.
Now the equation is balanced.
4Fe + 3O2 → 2Fe2O3
For eacht 4 moles Fe consumed, we will produce 2 moles Fe2O3
The mole ration is 4:2 (option 1)
Answer:
Can you do it in english please don't understand Spanish much. thanks
