Fill with 100 g H2o 200g 55 g Na CO The can is equipped with an outer jacket con

Question

Fill with 100 g H2o 200g 55 g Na CO The can is equipped with an outer jacket containing sodium carbonate (Na CO), which dissolves in water rapidly and endothermically Na2Co,(s) 2 Na (a)+ Co,2(a?) AH 67.7 kJ The user adds water to the outer jacket, and the heat absorbed in the chemical reaction chills the drink. The can contains 200 g of drink, the jacket contains 55 g of Na2CO3, and 100 g of water are to be added. If the initial temperatures of the can and the water are 35 C on a summer day, what is the coldést temperature that the drink can reach? The can itself has a heat capacity of 40 1PC. Assume that the Na2CO3 solution and the drink both have the same heat capacity as pure water, 4.184J g °c Hint: treat this like a calorimetry problem. oc

Explanation / Answer

from equation, 1 mol Na2CO3 = 67.7 kj

no of mol of Na2CO3 = 55/106 = 0.52 mol

amount of heat absorbed during the process = 67.7*0.52/1

                          = 35.204 kj

heal absorbed by Na2CO3 solution = heat lost by beverage + can

     35.2*10^3 = m*s*DT1 + C*DT1

m = mass of beverage = 200 g

s = specific heat of beverage = 4.184 j/g.c

DT1 = 35-x

C = heat capacity of can = 40 j/c

35.2*10^3 = 200*4.184*(35-x) + 40*(35-x)

x = final temperature of can = -5.146 c

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