The value of Change in heat for the reaction below is -790 KJ. Calculate the enthalpy change accompanying the reaction of .95 g of S.

2S(s) + 3 O2 --> 2 SO3(g)

The answer is -12 KJ this is from mastering chem.

To calculate the enthalpy change accompanying the reaction of 0.95 g of S, we need to use stoichiometry and the given value of change in heat.

First, we need to determine the moles of S in 0.95 g. To do this, we need to know the molar mass of S, which is 32.06 g/mol.

Number of moles of S = Mass of S / Molar mass of S
= 0.95 g / 32.06 g/mol
= 0.0296 mol (approximately)

Next, we need to use the stoichiometry of the balanced equation to find the moles of SO3 produced. From the balanced equation:
2 moles of S react to form 2 moles of SO3

Therefore, for every 2 moles of S reacted, 2 moles of SO3 are produced. This gives us:

Number of moles of SO3 = Number of moles of S x (2 moles of SO3 / 2 moles of S)
= 0.0296 mol x (2/2)
= 0.0296 mol

Now, we can calculate the enthalpy change accompanying the reaction of 0.95 g of S using the given value of change in heat.

Enthalpy change = Change in heat / Number of moles of SO3
= -790 KJ / 0.0296 mol
= -26,689.19 KJ/mol (approximately)

Therefore, the enthalpy change accompanying the reaction of 0.95 g of S is -26,689.19 KJ/mol.