Answer
Q1= energy needed to warm the ice from -20 degree C to 0 degree C
Q1= mass of ice*specific heat of ice *temperature change
= (10 g)*(2.1 J/gC)*(20 degree C)= 420 J
Q2= energy needed to phase change of H2O(from solid to liquid )
Q2= mass of H2O* latent heat of fusion of water
= (10 g)*(334 J/g)= 3340 J
Q3= energy needed to warm the water from 0 to 10 degree C
Q3= mass of water *specific heat of water *temperature change
= (10 g)*(4.184 J/gC)*(10)= 418.4 J
Q= Q1+Q2+Q3 = 420+3340+418.4 = 4178.4 J
1 kcal = 4184 J
The answer is 1 Kcal option (C)
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