Problem: Suppose you place 0.0300 g of magnesium chips in a coffee-cup calorimeter and then add 100 0 ml. of 1.00 M HCl. The reaction that occurs isMg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq)The temperature of the solution increases from 22.56 °C (295.71 K) to 23.91 °C (297.06 K). What is the enthalpy change (kJ/mol)  for the reaction per mole of Mg? Assume a specific heat capacity of the solution is 4.20 J/g • K and the density of the HCI solution is 1.00 g/mL.

90% (5 ratings)
90% (5 ratings)
Problem Details

Suppose you place 0.0300 g of magnesium chips in a coffee-cup calorimeter and then add 100 0 ml. of 1.00 M HCl. The reaction that occurs is

Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq)

The temperature of the solution increases from 22.56 °C (295.71 K) to 23.91 °C (297.06 K). What is the enthalpy change (kJ/mol)  for the reaction per mole of Mg? Assume a specific heat capacity of the solution is 4.20 J/g • K and the density of the HCI solution is 1.00 g/mL.

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Our tutors have indicated that to solve this problem you will need to apply the Constant-Pressure Calorimetry concept. You can view video lessons to learn Constant-Pressure Calorimetry Or if you need more Constant-Pressure Calorimetry practice, you can also practice Constant-Pressure Calorimetry practice problems .

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Based on our data, we think this problem is relevant for Professor Sempertegui's class at FAU.