EXPERIMENT 10.B Enthalpy Combining these three equations yields the required equ

Question

EXPERIMENT 10.B Enthalpy Combining these three equations yields the required equation: Mg(s) + ½ 02(g) --> MgO(s) that running an equation in the opposite direction simply changes the sign of the heat of formation. Weigh 0.6 g of magnesium and place in the alorimeter. Add the HCI and report the highest temperature reached within several minutes of stirring. Then eter and again measure 60 mL of IM HCI. Weigh 1.0 g of MgO and place in the Be aware Obtain 60 ml of IM HCI and measure its temperature. Weigh 0.6 g of magnesium and pla clean the calorimeter and again measure 60 mL of 1M calorimeter. Add the HCl solution and then measure the highest temperature as above. CI. Weieh uo g of Mgo and place in the

Explanation / Answer

Given mass of magnesium = 0.602 gms

Moles of Mg = mass / molecular weight = 0.025 moles

delta T = 66.9 - 24 = 42.9 C

Heat gained by solution = m*C*delta T = 0.602*1*42.9 = 25.82 J [C is assumed 1 ]

heat gained by the solution = - heat lost by the reaction = - 25.82J

Heat of solution = Heat gained by the solution / moles of Mg = 1032 J/mole

Heat of solution = 1.032 KJ/mole

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