/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Q4E Question: Calculate the heat cap... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 5: Q4E (page 268)

Question: Calculate the heat capacity, in joules and in calories per degree, of the following:

(a) 28.4 g of water

(b) 1.00 oz of lead

Short Answer

Expert verified

The heat capacity in joules:

  1. 28.4 g of water = 118.2\(\frac{J}{{{}^0C}}\)
  2. 1.00 oz of lead =3.68 \(\frac{J}{{{}^0C}}\)

The heat capacity in calories:

  1. 28.4 g of water =28.38 \(\frac{{cal}}{{^0C}}\)
  2. 1.00 oz of lead =0.879 \(\frac{{cal}}{{^0C}}\)

Step by step solution

01

Heat capacity

The heat capacity of a substance can be calculated by the formula H = mc, where 鈥渕鈥� is the mass of the substance and 鈥渃鈥� is its specific heat capacity.

02

Heat capacity of water in joules

From table 5.1, we know that the specific heat capacity of water is 4.184J/g鈩�.

Mass of the water = 28.4 g (given).

Therefore, the heat capacity of 28.4 g of water in joules = 28.4 \( \times \)4.184

= 118.82\(\frac{J}{{{}^0C}}\)

03

Heat capacity of water in calories per degree

1 calorie = 4.186 J.

The heat capacity of 28.4 g of water in calories is evaluated as:

=\(\frac{{118.82}}{{4.186}}\frac{{cal}}{{^0C}}\)

=28.38 \(\frac{{cal}}{{^0C}}\)

04

Step 4:Heat capacity of lead in joules

From table 5.1, we know that the specific heat capacity of lead is 0.130J/g鈩�.

The mass of the lead = 1 oz (given)

The mass of the lead in grams = 28.35\( \times \)1 = 28.35 g.

Therefore, the heat capacity of 28.35 g of lead in joules = 0.130\( \times \)28.35

= 3.68 \(\frac{J}{{{}^0C}}\)

05

Heat capacity of lead in calories per degree

1 calorie = 4.186 J.

The heat capacity of 28.35 g of lead in calories is calculated as:

\(\begin{array}{c} = \frac{{3.68}}{{4.186}}\\ = 0.879\frac{{cal}}{{^0C}}\end{array}\)

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Would the amount of heat measured for the reaction in example 5.5be greater, lesser, or remain the same if we used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.

Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4掳C causes the temperature to rise to 25.8掳C. What is the approximate amount of heat involved in the dissolution, assuming the heat capacity of the resulting solution is 4.18 J/g掳C? Is the reaction exothermic or endothermic?

Water gas, a mixture of \({{\bf{H}}_{\bf{2}}}\) and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon:\({\bf{C}}\left( {\bf{s}} \right){\bf{ + }}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right) \to {\bf{CO}}\left( {\bf{g}} \right){\bf{ + }}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right)\).

(a) Assuming that coke has the same enthalpy of formation as graphite, calculate \({\bf{\Delta H}}_{{\bf{298}}}^{\bf{0}}\)for this reaction.

(b) Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst:\({\bf{2}}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right){\bf{ + CO}}\left( {\bf{g}} \right) \to {\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\left( {\bf{g}} \right)\).

Under the conditions of the reaction, methanol forms as a gas. Calculate \({\bf{\Delta H}}_{{\bf{298}}}^{\bf{0}}\)for this reaction and for the condensation of gaseous methanol to liquid methanol.

(c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g).

Calculate the heat capacity, in joules and in calories per degree, of the following:

(a) 45.8 g of nitrogen gas

(b) 1.00 pound of aluminum metal

A 248-g piece of copper initially at 314 掳C is dropped into 390 mL of water initially at 22.6 掳C. Assuming that all heat transfer occurs between copper and water, calculate the final temperature.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.