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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The energy required to melt 1.00 g of ice at 0 °C is 333 J. If one ice cube has a mass of 62.0 g and a tray contains 16 ice cubes, what quantity of energy is required to melt a tray of ice cubes to form liquid water at 0 °C?

Interpretation Introduction

Interpretation:

Energy required to melt ice at definite mass has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1k.Energy gained or lost can be calculated using the below equation.

  q=C×m×ΔT

Where,

  q= energy gained or lost for a given mass of substance (m),

  C =specific heat capacity

  ΔT= change in temperature

Explanation

Given,

  Mass of ice is =1g

  Heat energy =333J

Assume the sum of two energy quantities are zero.

To melt the mass of ice to form liquid water at 0oC

                                   q=333J/g×1g=333J

For one ice cube, mass is 62g

x

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