Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 52

It takes \(585 \mathrm{J}\) of energy to raise the temperature of \(125.6 \mathrm{g}\) mercury from \(20.0^{\circ} \mathrm{C}\) to \(53.5^{\circ} \mathrm{C}\). Calculate the specific heat capacity and the molar heat capacity of mercury.

Short Answer

Expert verified
The specific heat capacity of mercury is \(0.139 \frac{J}{g \cdot °C}\), and the molar heat capacity of mercury is \(27.88 \frac{J}{mol \cdot °C}\).

Step by step solution

01

List the given information

We know the following: - Energy (Q) = 585 J - Mass of mercury (m) = 125.6 g - Initial temperature (T1) = 20.0°C - Final temperature (T2) = 53.5°C
02

Calculate the temperature change

We need to find the change in temperature (ΔT) by subtracting the initial temperature (T1) from the final temperature (T2): ΔT = T2 - T1 ΔT = 53.5°C - 20.0°C ΔT = 33.5°C
03

Use the heat capacity formula to find the specific heat capacity

We have to find the specific heat capacity(c) using the formula: Q = mcΔT 585 J = (125.6 g)(c)(33.5°C) Rearrange the formula to solve for c: c = Q / (mΔT) c = 585 J / (125.6 g * 33.5°C) c = 0.139 J/(g•°C)
04

Calculate the molar heat capacity

Now, we need to find the molar heat capacity using the specific heat capacity and the molar mass of mercury. The molar mass of mercury is 200.6 g/mol. Molar heat capacity = Specific heat capacity * Molar mass of mercury Molar heat capacity = 0.139 J/(g•°C) * 200.6 g/mol Molar heat capacity = 27.88 J/(mol•°C) The specific heat capacity of mercury is 0.139 J/(g•°C), and the molar heat capacity of mercury is 27.88 J/(mol•°C).

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by quinone in certain enzymes allows plants to take water, carbon dioxide, and the energy of sunlight to create glucose. A \(0.1964-\mathrm{g}\) sample of quinone \(\left(\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{O}_{2}\right)\) is burned in a bomb calorimeter with a heat capacity of \(1.56 \mathrm{kJ} / \mathrm{C}\). The temperature of the calorimeter increases by \(3.2^{\circ} \mathrm{C}\). Calculate the energy of combustion of quinone per gram and per mole.

For the process \(\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{O}(g)\) at \(298 \mathrm{K}\) and 1.0 atm, \(\Delta H\) is more positive than \(\Delta E\) by 2.5 kJ/mol. What does the \(2.5 \mathrm{kJ} / \mathrm{mol}\) quantity represent?

Liquid water turns to ice. Is this process endothermic or exothermic? Explain what is occurring using the terms system, surroundings, heat, potential energy, and kinetic energy in the discussion.

A balloon filled with \(39.1 \mathrm{moles}\) of helium has a volume of \(876 \mathrm{L}\) at \(0.0^{\circ} \mathrm{C}\) and \(1.00 \mathrm{atm}\) pressure. The temperature of the balloon is increased to \(38.0^{\circ} \mathrm{C}\) as it expands to a volume of \(998 \mathrm{L}\), the pressure remaining constant. Calculate \(q, w,\) and \(\Delta E\) for the helium in the balloon. (The molar heat capacity for helium gas is \(20.8 \mathrm{J} /^{\circ} \mathrm{C} \cdot \mathrm{mol}.\))

At \(298 \mathrm{K},\) the standard enthalpies of formation for \(\mathrm{C}_{2} \mathrm{H}_{2}(g)\) and \(\mathrm{C}_{6} \mathrm{H}_{6}(l)\) are \(227 \mathrm{kJ} / \mathrm{mol}\) and \(49 \mathrm{kJ} / \mathrm{mol},\) respectively. a. Calculate \(\Delta H^{\circ}\) for $$\mathrm{C}_{6} \mathrm{H}_{6}(l) \longrightarrow 3 \mathrm{C}_{2} \mathrm{H}_{2}(g)$$ b. Both acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) can be used as fuels. Which compound would liberate more energy per gram when combusted in air?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

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.

Sign-up for free