   # Suppose that only two 45-g ice cubes had been added to your glass containing 5.00 × 10 2 mL of tea (see Study Question 78). When thermal equilibrium is reached, all of the ice will have melted, and the temperature of the mixture will be somewhere between 20.0 ° C and 0 °C. Calculate the final temperature of the beverage. ( Note : The 90 g of water formed when the ice melts must be warmed from 0 °C to the final temperature.) ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 5, Problem 79GQ
Textbook Problem
273 views

## Suppose that only two 45-g ice cubes had been added to your glass containing 5.00 × 102 mL of tea (see Study Question 78). When thermal equilibrium is reached, all of the ice will have melted, and the temperature of the mixture will be somewhere between 20.0 °C and 0 °C. Calculate the final temperature of the beverage. (Note: The 90 g of water formed when the ice melts must be warmed from 0 °C to the final temperature.)

Interpretation Introduction

Interpretation:

At thermal equilibrium the final temperature of the beverage 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 of Solution

Let the amount of ice melted=x

Assume qwater=-qice

Given,

The specific heat capacity is 4.2J/gK

Mass of the tea is 500g

Mtea×C×ΔTtea=-[(Mice×333J/g)+Mice×C×(F-273

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