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# If 1.10 g of steam at 100.0 °C condenses into 38.5 g of

ISBN: 9780321910295 34

## Solution for problem 104P Chapter 12

Introductory Chemistry | 5th Edition

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Problem 104P

PROBLEM 104P

If 1.10 g of steam at 100.0 °C condenses into 38.5 g of water, initially at 27.0 °C, in an insulated container, what is the final temperature of the entire water sample? Assume no loss of heat into the surroundings.

Step-by-Step Solution:

Solution 104P

Here, we have to calculate the final temperature of the entire water sample.

Step 1:

Heat capacity of a system is given by

q = m x Cs x T  …………..(1)

Where, Heat ( q ), Mass ( m ), Temperature ( T ), and Specific Heat Capacity of a Substance ( Cs ) respectively.

Step 2:

Given that

For hot system

M = 1.10 g

Ti = 100.0 °C

Cs = 4.18 J/g . °C

Similarly for cold system

M = 38.5 g

Ti = 27 °C

Cs = 4.18 J/g . °C

Tf =?

Step 3 of 3

##### ISBN: 9780321910295

This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 104P from chapter: 12 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 104P from 12 chapter was answered, more than 397 students have viewed the full step-by-step answer. This full solution covers the following key subjects: Water, insulated, container, entire, final. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The answer to “If 1.10 g of steam at 100.0 °C condenses into 38.5 g of water, initially at 27.0 °C, in an insulated container, what is the final temperature of the entire water sample? Assume no loss of heat into the surroundings.” is broken down into a number of easy to follow steps, and 40 words.

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