Question

1. solution is made by dissolving 20.0 g of magnesium metal in enough water to form magnesium hydroxide and hydrogen at constant pressure of 785 torr and 25.0 °C according to the following unbalanced chemical reaction:

Mg(s) + H₂O (l) → Mg(OH)₂ (aq) + H₂ (g)

Compound	∆H°f (kJ/mole)
Mg(OH)2 (aq)	-924.5
H2O(l)	-285.8
H2(g)	0.00
Mg(s)	0.00

Calculate ∆H° of the reaction in kJ/mol Mg.

Calculate ∆H° of the reaction in kJ/gram of Mg

If the initial volume of the reaction is 2.00 L and the volume of the reaction expands at 25.0 °C and 785.0 torr. Calculate the work that is produced by the reaction (in kJ).

Calculate the change in internal energy (DE).

The internal energy calculated above is _______.

The amount of heat that is emitted by the reaction is used to warm 2.20 kg of sand (C_sand=0.84 J/g.°C) at 25.0°C.

Determine the final temperature of the sand.

Answer 1

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