0.15g Mg reacted with 50ml 1M HCL in a calorimeter: The calorimeter constant is 9.3 Mg (s) + 2HCL (aq) ---> Mg2+ (aq) + 2Cl- (aq) + H2 (g)
Mass of the empty calorimeter (g) 18.600g
Initial temperature of the calorimeter (°C) 21.5 C
Maximum temperature in the calorimeter from the reaction (°C) 34.5C
Calculate delta T by subtracting (b) from (c) (°C) delta T = Tmaximum - Tinitial 13.0C
Mass of the calorimeter and its contents after the reaction (g) 68.738g
Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e) 50.138g
Calculate the moles of Mg reacted (MW = 24.305 g/mole) 0.006mol
1) Calculate the heat released into the solution for the reaction, according to:
Q = (Ccal * deltaT) + (mass of water * Cp(water) * deltaT)
2) Find the molar heat of reaction for each experiment in units of Kilo-Joules / (mole of Mg) by dividing the heat of reaction by the moles of Mg used. Show all work and include units for all values.
3) Using your calculated value for molar heat of reaction, how much heat would be given off in kilojoules if 3.0 grams of magnesium were to react with excess hydrochloric acid. Show work for your calculation.