Answer:
Max. work done in 60 g of copper plated out is 200472.14 J
Explanation:
Given cell reaction is:

Standard reduction potential of Zn electrode (
) is 0.763 V.
Standard reduction potential of Cu electrode (
) is -0.337 V.
Copper acts as cathode and Zinc acts as anode.
Cell potential (E) = E° cathode - E° anode
= 0.763 - (-0.337)
= 1.10 V
formula for the work done is as follows:

Here, n is no. of electron involved in the reaction.
F(Faraday's constant) = 96500
In the given reaction, n = 2

Therefore, 212300 J work is done by reducting 1 mol of copper.
Copper given is 60 g.
Molecular mass of copper is 63.54 g/mol.

Max. work done in 60 g of copper plated out is:

There are 100cm in a metre.
16.45=16+0.45.
Therefore 16.45m=1600cm+45cm=1645cm.
Answer:
How many hydrogen MOLECULES are needed to produce 2 molecules of water (H2O)?
Explanation:
Answer:

Explanation:
Assume the reaction is the combustion of propane.
Word equation: propane plus oxygen produces carbon dioxide and water
Chemical eqn: C₃H₈(g) + O₂(g) ⟶ CO₂(g) + H₂O(g)
Balanced eqn: C₃H₈(g) + 5O₂(g) ⟶ 3CO₂(g) + 4H₂O(g)
(a) Table of enthalpies of formation of reactants and products

(b)Total enthalpies of reactants and products

ΔᵣH° is negative, so the reaction is exothermic.
Answer:
4 moles of NH3 will be produced
Explanation:
The reaction expression is given as:
N₂ + 3H₂ → 2NH₃
We have to check that the equation of the reaction is balanced.
Then;
if 2 mole of N₂ reacts;
1 mole of N₂ will react with 3 mole of H₂ to produce 2 mole of NH₃
2 mole of N₂ will react with (2x3)mole of H₂ to produce (2x2)mole of NH₃
6mole of H₂ to produce 4 mole of NH₃