50 g of ice, at 0 oC, is added to 500 g of water at 75 o What is the final temperature? Cice = 2.093 J/g-oC, cH2O = 4.186 J/g-oC.

The final temperature of the mixture is 71.43 ⁰C

Explanation:

Given;

mass of ice, m₀ = 50 g

initial temperature of the ice, t₀ = 0 ⁰C

mass of water, m₁ = 500 g

initial temperature of water, t₁ = 75 ⁰C

specific heat capacity of ice, C₀ = 2.093 J/g⁰C

specific heat capacity of water, C₁ = 4.186 J/g⁰C

Let the final temperature of the mixture = T

The heat lost by the water = The heat gained by the ice

m₁c₁ (75 - T) = m₀c₀ (T - 0)

500 x 4.186 x (75 - T) = 50 x 2.093 x T

156975 - 2093T = 104.65T

156975  = 104.65T   +   2093T

156975  = 2197.65T

T = 156975 / 2197.65

T = 71.43 ⁰C

Therefore, the final temperature of the mixture is 71.43 ⁰C

the increase of protons   hope this

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