Suppose you place 0.0400 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 21.66 °C (294.81 K) to 23.46 °C (296.61 K). What is the enthalpy change 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 HCl solution is 1.00 g/mL.
The heat of a substance is given as :
Mass of Mg = 0.0400 g
Mass of HCl solution = 100.0 mL
Molarity of HCl solution = 1.00 M
Initial temperature, T1 = 294.81 K
Final temperature, T2 = 296.61 K
Specific heat capacity of solution, Csol = 4.20 J/g.K
Density of HCl solution = 1.00 g/mL
Moles of Mg (n) can be calculated as :
The mass of HCl solution can be calculated as :
△T = T2 – T1 = 296.61 K – 294.81 K = 1.8 K...
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