# What are the steps to this basic thermodynamics equation?

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What are the steps to solving this problem?

Honestly I'm not looking for the answer, I want to actually know the steps on how to solve this sort of problem. Thanks :)

A 0.582-g sample of Mg reacts with excess 1.0 M HCl (60.0 mL) according to the procedure used in this experiment. The initial and final temperatures were 24°C and 68°C. What is the ∆H of the reaction per mole of magnesium? Assume that the specific heat capacity for the solution is 4.187 J/deg∙g and that the density of the 1.0 M HCl is 1.00 g/mL. (Hints: the magnesium contributes to the mass of the solution)

What are the steps to solving this problem?

Honestly I'm not looking for the answer, I want to actually know the steps on how to solve this sort of problem. Thanks :)

A 0.582-g sample of Mg reacts with excess 1.0 M HCl (60.0 mL) according to the procedure used in this experiment. The initial and final temperatures were 24°C and 68°C. What is the ∆H of the reaction per mole of magnesium? Assume that the specific heat capacity for the solution is 4.187 J/deg∙g and that the density of the 1.0 M HCl is 1.00 g/mL. (Hints: the magnesium contributes to the mass of the solution)

This is how I would proceed:

Write down the actual reaction. You should anticipate a single replacement reaction when magnesium, a monatomic substance, reacts with hydrochloric acid, a diatomic substance:

- Examine your available variables and determine which equation they fit into.

That ought to bring to mind:

where

- Using the information you were given, determine how to find these variables.

We are under constant pressure, as you can now see, so this relationship is valid:

Therefore, to calculate the molar enthalpy:

- Work out your concluding equation:

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Sure, could you please provide the specific basic thermodynamics equation you're referring to?

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