Part C to heat 34.2 g of copper from 122° C to 227 °C Express your answer using three significant figures. J Submit Previous Answers Completed; correct answer withheld by instructor Part D to heat 34.2 g of copper from 122° C to 227 °C Express your answer using three significant figures. cal

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help on part C and part D

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Test Chapter
Item 13
Use the heat equation
calories, for each of the following (see the table):
(Figure 1)
calculate the energy, in joules and
Part C
to heat 34.2 g of copper from 122° C to 227 °C
Express your answer using three significant figures.
J
Submit
Previous Answers
Completed; correct answer withheld by instructor
Part D
Figure
1 of 1
to heat 34.2 g of copper from 122°C to 227°C
Substance
cal/g °C
J/g °C
Express your answer using three significant figures.
Elements
Aluminum, Al(s)
0.214
0.897
cal
Copper, Cu(s)
0.0920
0.385
Gold, Au(s)
0.0308
0.129
Submit
Previous Answers
Iron, Fe(s)
0.108
0.452
Silver, Ag(s)
0.0562
0.235
Completed; correct answer withheld by instructor
Titanium, Ti(s)
0.125
0.523
Compounds
Ammonia, NH3(g)
0.488
2.04
Part E
Ethanol, C,H;OH(!)
0.588
2.46
Sodium chloride, NaCI(s)
0.207
0.864
lost when 12.3 g of ethanol, C2 H, OH, cools from 50.0 °C to -42.0°C
Water, H,O(!)
1.00
4.184
Express your answer using three significant figures.
Water, H20(s)
0.485
2.03
J
Transcribed Image Text:Safari File Edit View History Bookmarks Window Help session.masteringchemistry.com Test Chapter Item 13 Use the heat equation calories, for each of the following (see the table): (Figure 1) calculate the energy, in joules and Part C to heat 34.2 g of copper from 122° C to 227 °C Express your answer using three significant figures. J Submit Previous Answers Completed; correct answer withheld by instructor Part D Figure 1 of 1 to heat 34.2 g of copper from 122°C to 227°C Substance cal/g °C J/g °C Express your answer using three significant figures. Elements Aluminum, Al(s) 0.214 0.897 cal Copper, Cu(s) 0.0920 0.385 Gold, Au(s) 0.0308 0.129 Submit Previous Answers Iron, Fe(s) 0.108 0.452 Silver, Ag(s) 0.0562 0.235 Completed; correct answer withheld by instructor Titanium, Ti(s) 0.125 0.523 Compounds Ammonia, NH3(g) 0.488 2.04 Part E Ethanol, C,H;OH(!) 0.588 2.46 Sodium chloride, NaCI(s) 0.207 0.864 lost when 12.3 g of ethanol, C2 H, OH, cools from 50.0 °C to -42.0°C Water, H,O(!) 1.00 4.184 Express your answer using three significant figures. Water, H20(s) 0.485 2.03 J
Expert Solution
Step 1

Heat required for raising the temperature of a substance of mass m from one point to another can be calculated buy the following formula.

Q=mcTQ=amount of heat requiredm=massc=specific heat of substance under considerationT=temperature difference

Step 2

C) Mass of copper is given as 34.2 g.

Temperature difference can be calculated as follows.

T=Tfinal-Tinitial=227 0C-122 0C=105 0C

Required unit for specific heat is J/g 0C because we need the answer in joules.

Now we can calculate the amount of heat required.

Q=mcT=34.2 g×0.385 Jg 0C×105 0C=1382.5 J=1380 J

Hence the amount of heat required is 1380 J.

Hence the amount of heat required is 1380 J.

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