Mg reacts with H+ (aq) according to Mg(s)+2H+(aq)→Mg2+(aq)+H2(g) Suppose that 0.524 g of Mg is reacted with 60.o ml of 1.0 M H+(aq). Assume that the density of the H+ (aq) solution os 1.00 g/ml,and that its specific heat capacity equals that of water. Theinitial and final temperatures are 22.0 degree celsius and 65.8degree celsius. a) Is the reaction endothermic or exothermic? b) Calculate △H of of th reaction. Use correct sigs andgive units. c) Calculate the △H of the reaction per mole of magnesium.

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Mg reacts with H+ (aq) according to  Mg(s)+2H+(aq)→Mg2+(aq)+H2(g)  Suppose that 0.524 g of Mg is reacted with 60.o ml of 1.0 M H+(aq). Assume that the density of the H+ (aq) solution os 1.00 g/ml,and that its specific heat capacity equals that of water. Theinitial and final temperatures are 22.0 degree celsius and 65.8degree celsius.  a) Is the reaction endothermic or exothermic?  b) Calculate △H of of th reaction. Use correct sigs andgive units.  c) Calculate the △H of the reaction per mole of magnesium.

Lacey-May Snyder · Accepted Answer

Mg(s)+2H+(aq)→Mg2+(aq)+H2(g) Part a) Reaction of Metallic magnesium with acid is an exothermic reaction Part b) We have, Moles of Mg=MassMolar mass=0.52424.305=0.02156 mol Now, mass of the solution = Mass of water + Mass of Mg = 0.524 + 60.0 = 60.524 g q=−mc△T Where q is the heat released c is the specific heat △T is the temperature change Therefore, q=60.524×4.184×(65.8−22.0)=−11091.6 J=−11.09 KJ Part c) Heat released per mole of Mg=(−11091.60.02156)=−514KJmol

Mg reacts with H+ (aq) according to Mg(s)+2H+(aq)\to Mg_2+(aq)+H_2(g) Suppose that 0.524 g of Mg is reacted with 60.o ml of 1.0 M H+(aq). Assume that

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