💬 👋 We’re always here. Join our Discord to connect with other students 24/7, any time, night or day.Join Here!

Get the answer to your homework problem.

Try Numerade free for 7 days

Like

Report

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

a) $118.826 \mathrm{j} /^{\circ} \mathrm{C}, 28.4 \mathrm{cal} /^{\circ} \mathrm{C}$b) $3.685 \mathrm{j} /^{\circ} \mathrm{C}, 0.880 \mathrm{cal} /^{\circ} \mathrm{C}$

01:48

Aadit S.

02:48

Ronald P.

Chemistry 101

Chapter 5

Thermochemistry

Rice University

University of Maryland - University College

University of Toronto

Lectures

02:29

Chemistry is the science o…

04:42

In chemistry and physics, …

09:52

Use the heat equation to c…

12:26

09:33

A piece of lead with a mas…

12:29

04:10

In the LaboratoryA pie…

03:13

Calculate the final temper…

00:31

Calculate the amount of en…

04:18

Calculate the quantity of …

01:36

06:11

Calculate the heat change …

02:12

06:30

06:19

(a) What is the specific h…

05:36

02:34

How much heat, in joules a…

01:12

How much energy in calorie…

02:25

It takes $880 \mathrm{J}$ …

04:11

How much energy in kilojou…

Let's find the heat capacity and then jewels in and in calories per degree of the following. Let's start with R28 gram 28.4 grams of water. So how do I find the heat capacity basically the heat capacity kind of in the definition, in the word itself, the definition is in the word itself is how much heat. Mhm. How much he? So in this case we're talking jewels or not degrees Celsius, silly jewels or calories that a certain amount of substance, certain mass. So this isn't gramps of a substance. Right, What can hold? Yeah, Okay, so for a water, what we need here is to figure out how much heat one g holds so to speak And then we can extrapolate that to 28.4 rooms. So we're going to use a number called the specific heat. The specific heat of water which is basically how many jewels it takes to heat. A coward heat. Sorry, a degree of water. Heat a gram of water. Heat a gram of water by one degree. So hit one g of something in this case of water. Bye. One degree Celsius. The energy required to do that to heat the substance. So what is the specific heat of water? The specific heat of water in jewels is 4.14.186 jules, her graham degree Celsius. So let's break this down a bit. This means it takes 4.186 jewels To heat one g of water. One degree Celsius. So to increase the heat of water by one degree To increase the heat of water of one g of water by one degree. You need 4.186 jewels and 4.186 jules is equal to one calorie. Keep writing the degree sign one calorie. Okay, so then let's calculate this. So we have 28.4 g of water and we're trying to figure out how much how many jewels basically that can take. So as you can see, our grams will cancel out because there's one of the numerator and one in the denominator. So this will leave us with jules per degree Celsius, which is exactly what the question is asking for. And when we multiplied 28.4 times 4.186, we get 118.89, 118.89 jewels. Okay, so then if we divide that number by that number by 4.186 which is one Calorie which is one jewel, so Which is sorry 4.186 jewels equal to one calorie. We'll get that. This is equal to 28.4 calories per degree Celsius. So these are our two answers for part A. Okay, now for part B, Part B, which is 1, 1 out of that. Yeah. Okay. one ounce of lead. What is the specific heat of lead? Yeah. Well the specific heat which is represented by the sea here is 0.44 jules her telegram. How jules? Her kilogram. So then we have to convert oz two kg. So let's do that. That's just plug this in. One ounce. Lead. One ounce Is equal to 0.02 8 3, 0.0 283 kg. And one kg should be pretty. three C. Okay, and then let's plug this specific heat in there. And sure enough, if we just go through and cancel our units out, just to be sure we're doing this right, we'll end up with jules per degree Celsius, which is exactly what we want. And then we'll also convert that to calories. Once we get jules. So what is that? Your zero 283, Time 0.44 is 0.0124, 0.0124 Jewels per degree C. So what this means is that it takes barely any jewels. Only 0.0124. To heat This much lead up by 1°. So water holds a heck of a lot more heat missing. Okay then we want to convert this to calories. Remember that that one calorie is equal to 4.186 jules. one calorie equals 4.186 jewels. So when we do this, we want to divide this number to your point 124 By 4.86. And we're going to get an even smaller number. We're going to get 0.00256 0.00256 calories per degree Celsius. To heat up this one ounce of lead. This is how many jules and calories of energy it would take to heat it up per degree. Okay, so to solve these kinds of problems, you will need the specific heat of each substance and then the conversion between jules and calories and all the conversions in between here and then this is how you can solve this problem. Remember. Don't look out for Sig figs here. Um looks like you have three Sig figs each. So make sure that you actually change this one too 1, 19 28.4 still works and this one works and this one works. You can change these scientific notation if you'd like to, but this works just fine. And this is how you solve this kind of problem.

View More Answers From This Book

Find Another Textbook

Numerade Educator

Chemistry is the science of matter, especially its chemical reactions, but a…

In chemistry and physics, matter is any substance that has mass and takes up…

Use the heat equation to calculate the energy for each of the following (see…

Use the heat equation to calculate the energy, in joules and calories, for e…

A piece of lead with a mass of $27.3 \mathrm{g}$ was heated to $98.90^{\circ…

In the LaboratoryA piece of lead with a mass of $27.3 \mathrm{g}$ was he…

Calculate the final temperature that results when (a) a12.6 g sample of …

Calculate the amount of energy required (in calories) to heat 145 g of water…

Calculate the quantity of heat, in kilojoules, (a) required to raise the tem…

Calculate the heat change at $100^{\circ} \mathrm{C}$ for each of the follow…

Calculate the amount of energy required (in joules) to heat 2.5 $\mathrm{kg}…

Calculate the quantity of heat required to increase the temperature of 100 $…

(a) What is the specific heat of liquid water? (b) What is the molar heat ca…

Calculate the heat change at $0^{\circ} \mathrm{C}$ for each of the followin…

How much heat, in joules and in calories, is required to heat a $28.4-\mathr…

How much energy in calories is required to raise the temperature of 200 g of…

It takes $880 \mathrm{J}$ to raise the temperature of $350 \mathrm{g}$ of le…

How much energy in kilojoules is released when 7.55 $\mathrm{g}$ of water at…

05:46

Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select t…

01:26

According to one theory, the pressure of a gas increases as its volume decre…

09:51

Predict and test the behavior of ? particles fired at a Rutherford atom mode…

00:33

Is a meter about an inch, a foot, a yard, or a mile?

01:22

The volume of a sample of oxygen gas changed from 10 mL to 11 mL as the temp…

02:27

Open the Build an Atom simulation (http://openstaxcollege.org/l/16PhetAtomBl…

Give the number of protons, electrons, and neutrons in neutral atoms of each…

00:37

An FM radio station found at 103.1 on the FM dial broadcasts at a frequency …

01:46

FM-95, an FM radio station, broadcasts at a frequency of $9.51 \times 10^{7}…

01:33

How are the molecules in oxygen gas, the molecules in hydrogen gas, and wate…