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Calculate the amount of heat needed to convert 230.0 g of ice at -10.0ºC to liquid water at 10.0ºC.

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The heat required to raise the temperature of ice from  -10.0ºC to 10.0ºC is 22.2 KJ.

The heat needed to convert 230.0 g of ice at -10.0ºC to liquid water at 10.0ºC is the sum of the latent heat of fusion of ice and the heat required to raise the temperature of the resulting water to.

Hence, the heat required is obtained from;

H = Heat required to raise the temperature from  -10.0ºC to 0ºC + Heat required to convert ice to water + Heat required to raise the temperature of water from 0ºC to 10.0ºC

H =[0.23 ×  2090 × (0 - (-10.0))] + [0.23 ×  33600] + [0.23 × 4186 × ( 10 - 0)]

H = 4807 + 7728 + 9627.8

H = 22.2 KJ

Learn more: https://brainly.com/question/20339399

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