A. calculate the quantity of heat released when 1.00 g of sulfur is burned in oxygen. b. calculate the quantity of heat released when 0.501 mole of sulfur is burned in air. c. what quantity of energy is required to break up 1 mole of so2(g) into its constituent elements?

A) 9.25 KJ.

B) - 148.296 KJ.

C) 296 KJ/mol.

Explanation:

For the reaction: S(s) + O2(g) → SO2(g), ΔH = -296 KJ/mol

A) The number of moles in 1.00 g of S is

n = mass/atomic mass = (1.00 g) / (32.00 g/mol) = 0.03125 mole

So, the quantity of heat when 1.00 g of sulfur burned in oxygen = ΔH of the reaction for 1.0 mole x no. of moles = (-296 KJ/mol) x (0.03125 mole) = 9.25 KJ.

B) The quantity of heat released when 0.501 mole of sulfur is burned in air = ΔH of the reaction for 1.0 mole x no. of moles = (-296 KJ/mol) x (0.501 mol) = - 148.296 KJ.

C) The quantity of energy is required to break up 1.0 mole of SO2(g) into its constituent elements = 296 KJ/mol.

It is the same that the amount of energy released when 1.0 mole of S is burned in oxygen.

The process of formation (burning of S) is exothermic.

On the other hand, the reverse operation (breakdown) must be endothermic (and therefore a positive energy change) = 296 KJ/mol.

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.