I\'ve given the answers for a, b, c, d, and e. Can you help with the answers for

ID: 533911 • Letter: I

Question

I've given the answers for a, b, c, d, and e. Can you help with the answers for f and g?

For the reaction of magnesium and HCl, the textbook value of H is -306.9 kJ/mol: Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g) H = -306.9 kJ/mol

a) A student dissolves 0.95 g of Mg in excess HCl. How much heat would be released by the reaction of 0.95 g of Mg with excess HCl? q = 12 kJ

b) Would this process be exothermic or endothermic? Exothermic

c) Based on your answer to b,would you expect the temperature of the solution (surroundings) to increase or decrease? Increase

d) Based on your answer to a-c, how much heat is absorbed by the surroundings? 12 kJ

e) If the HCl solution had a mass of 175.32 g. What temperature change would the student measure for the solution?

f) If the student measured the initial temperature of the solution as 18.2 °C, what would the final temperature be?

q = m × T × C

Where, q = heat absorbed by solution, 12000J

m = mass of solution ,175.32g

C = Specific heat of solution, 4.184J/mol K

T = ?

T = q/m × C

= 12000J /175.32g × 4.184(J/g )

= 16.36

f) If initial temperature of the solution is 18.2

Final temperature of the solution = 18.2 + 16.36 = 34.56

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