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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

You take a diet cola from the refrigerator and pour 240 mL of it into a glass. The temperature of the beverage is 10.5 °C. You then add one ice cube (45 g) at 0 °C. Which of the following describes the system when thermal equilibrium is reached?

(a) The temperature is 0 °C, and some ice remains.

(b) The temperature is 0 ° C, and no ice remains.

(c) The temperature is higher than 0 °C, and no ice remains.

Determine the final temperature and the amount of ice remaining, if any.

Interpretation Introduction

Interpretation:

The final temperature and amount of ice remaining 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

a) Cola and ice –system

b) Cola and solution of ice –system

c) Cola –system

Assume the sum of two energy quantities are zero.

Use the above equation to find out the sum of energy quantities.

               [Ccola×Mcola(Tfinal-Tinitial)+Cice×Mice(Tfinal-Tinitial)]=0

Substitute for the two energy quantities

4.2JK/L×240g(273K-283

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