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

View Video Answer

Like

Report

How much heat, in joules and in calories, is required to heat a $28.4-\mathrm{g}(1-\mathrm{oz})$ ice cube from $-23.0^{\circ} \mathrm{C}$ to $-1.0^{\circ} \mathrm{C} ?$

1310 joule, 313 cal

Chemistry 101

Chapter 5

Thermochemistry

University of Maryland - University College

Brown University

University of Toronto

Lectures

02:29

Chemistry is the science o…

04:42

In chemistry and physics, …

07:23

$\bullet$ How much heat is…

06:48

How much heat is required …

05:17

How much heat (in $\mathrm…

03:21

04:13

How much energy in kilojou…

09:05

03:40

. An ice-cube tray contain…

03:12

An ice-cube tray of neglig…

02:54

How much heat (in kJ) is r…

06:28

An ice-cule tray of neglig…

02:09

The heat energy required t…

03:38

03:17

When ice melts, it absorbs…

01:49

The energy required to mel…

02:25

Calculate the quantity of …

05:01

What mass of ice can be me…

05:03

How much energy is require…

05:40

From the data below, calcu…

05:54

How much heat is needed to…

05:33

How much heat is added to …

So today we're trying to figure out how much energy it's gonna take for us to heat 28.4 grams of ice from negative 23 degrees Celsius to negative one degree. Suskind's now in this equation, we're just gonna d'oh Q, which is heat equals. M s tells a T where m is the mass s is our specific heat. And then t is our change in temperature adult A T change in a temp. So we just have to solve for Q and we already have all of these values. So he was gonna equal 28.4 grams. This was a heat of ice is 2.11 Jules per grams degree Celsius. So that means it takes 2.11 Jules to heat one gram of ice by one degree Celsius and then Delta T is there's going to be our temperature final minus or temperature initial. So we end at a temperature of negative one, and we minus are starting time. Sure, which is 23 which means, like you is gonna equal 28.4 times 2.11 times 22. So if you really quick go. I've got into our calculators. That's gonna give us 1000 318.3 three jewels. And now it also wants to calculate this in calories. So I've included are converting factor for calories. A one calorie equals 4.2 jewels. So to convert from Jules into calories, we're just gonna divide by 4.2. So we divide this by 4.2. It's gonna give me 313 0.8 for calories. So those are two answers. 3 18 3 13.84 and 1318.33 Thanks for watching.

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…

$\bullet$ How much heat is required to convert 12.0 g of ice at $-10.0^{\cir…

How much heat is required to convert 12.0 g of ice at $-10.0^{\circ} \mathrm…

How much heat (in $\mathrm{kJ} )$ is required to warm 10.0 $\mathrm{g}$ of i…

How much heat is required to convert 18.0 g of ice at -10.0$^\circ$C to stea…

How much energy in kilojoules is needed to heat 5.00 $\mathrm{g}$ of ice fro…

How much heat (in $\mathrm{kJ}$ ) is needed to convert $866 \mathrm{g}$ of i…

. An ice-cube tray contains 0.350 $\mathrm{kg}$ of water at $18.0^{\circ} \m…

An ice-cube tray of negligible mass contains 0.350 $\mathrm{kg}$ of water at…

How much heat (in kJ) is required to warm 10.0 g of ice, initially at -10.0 …

An ice-cule tray of negligible mass contains 0.350 $\mathrm{kg}$ of water at…

The heat energy required to melt $1.00 \mathrm{g}$ of ice at $0^{\circ} \mat…

An ice-cube tray of negligible mass contains 0.290 kg of water at 18.0$^\cir…

When ice melts, it absorbs 0.33 kJ per gram. How much ice is required to coo…

The energy required to melt $1.00 \mathrm{g}$ of ice at $0^{\circ} \mathrm{C…

Calculate the quantity of heat required to convert $60.1 \mathrm{g}$ of $\ma…

What mass of ice can be melted with the same quantity of heat as required to…

How much energy is required to change a 40.0 -g ice cube from ice at $-10.0^…

From the data below, calculate the total heat (in $\mathrm{J}$ needed to con…

How much heat is needed to change $3.00 \times 10^{2} \mathrm{g}$ of ice at …

How much heat is added to $10.0 \mathrm{g}$ of ice at$-20.0^{\circ} \mat…

01:11

The amount of heat required to melt 2 lbs of ice is twice the amount of heat…

03:02

Identify each of the underlined items as a part of either the macroscopic do…

01:30

We refer to astronauts in space as weightless, but not without mass. Why?

03:08

How does an element differ from a compound? How are they similar?

04:43

The addition of 3.15 g of $\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{…

00:44

Which postulate of Dalton’s theory is consistent with the following observat…

01:16

Identify the postulate of Dalton’s theory that is violated by the following …

00:41

Classify each of the following changes as physical or chemical:(a) conde…

Classify each of the following changes as physical or chemical:(a) coal …

02:28

A 0.500 -g sample of $\mathrm{KCl}$ is added to 50.0 $\mathrm{g}$ of water i…