2. A sample of copper was heated to 120.0°C and then added to 200.0 g of water at 25.0 °C. The resulting mixture reached 26.5 °C. Knowing the specific heat capacity of copper is 0.387 J/g°C, calculate the mass of copper used. Hint: Think about energy transfers and draw a sketch.
2. A sample of copper was heated to 120.0°C and then added to 200.0 g of water at 25.0 °C. The resulting mixture reached 26.5 °C. Knowing the specific heat capacity of copper is 0.387 J/g°C, calculate the mass of copper used. Hint: Think about energy transfers and draw a sketch.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:2. A sample of copper was heated to 120.0°C and then added to 200.0 g of water at 25.0 °C. The resulting mixture
reached 26.5 °C. Knowing the specific heat capacity of copper is 0.387 J/g°C, calculate the mass of copper used.
Hint: Think about energy transfers and draw a sketch.

Transcribed Image Text:Selected Standard Molar Enthalpies of Formation
AH₁
AH;
AH₁
Substance (kJ/mol) Substance (kJ/mol) Substance (kJ/mol)
Al₂O3(s)
-1675.7 HBr(g)
CaCO3(s)
-1207,6 HCl(g)
CaCl₂(s)
Ca(OH)₂(s)
CCL₂(E)
CCL4(8)
CHCI ()
CH₂(g)
C₂H₂(g)
C₂H₁(g)
C₂H₂(g)
CzHs(g)
CH()
CH₂OH(E)
C₂H₂OH()
CO(g)
CO₂(g)
COCI₂(g)
+49.1 Fe₂O₂(8)
-239.2 Fe,O4(s)
-277.6 FeCl₂(s)
CH3COOH(E) –484.3 FeCls(s)
-110.5 FeS (8)
CS₂(e)
CS₂(g)
CrCla(g)
Cu(NO₂)₂ (8)
-795.4 HF(g)
-985.2 HCN(g).
-128.2 H₂O(E)
-95.7 H₂O(g)
CuO(s)
CuCl(s)
CuCl₂(s)
-134.1 H₂O₂(e)
-74.6 HNO (0)
+227.4 H₂PO4(s)
+52.4 H₂S(g)
-84.0 H₂SO4(e)
-103.8 FeO(s)
–36.3|NH(8)
-92.3 N₂H4(e)
-273.3 NH Cl(s)
+135.1 NH₂NO(s)
-285.8 NO(g)
-393.5 PbCl₂(s)
-219.1 MgCl₂(s)
+89.0 MgO(s)
+116.7 Mg(OH)2(s)
-556.5 HgS(s)
-241.8 NO₂(g)
-187.8 N₂O(g)
-174.1 N₂O(g)
1284.4 PH,(g)
-20.6 PCl₂(g)
814.0 P,O,(s)
-272.0 P4O₁0(s)
-824.2 KBr(s)
-1118.4 KCl(s)
-341.8 KCIO,(s)
-399.5 KOH(s)
-178.2 AgaCO₂ (s)
-359.4 AgCl(s)
-641.3 AgNO,(s)
-601.6 Ag S(s)
-924.5 SFB(g)
-58.2 SO₂(g)
-302.9 NaCl(s)
-411.2 SO₂(g)
-157.3 NaOH(s)
-425.6 SnCl₂(s)
-137.2 Na₂CO3(s)-1130.7 SnCl4(e)
-220.1
-45.9
+50.6
-314.4
-365.6
+91.3
+33.2
+81.6
+11.1
+5.4
-287.0
-2144.3
-2984.0
-393.8
-436.5
-397.7
-424.6
-505.8
-127.0
-124.4
-32.6
-1220.5
-296.8
-395.7
-325.1
-511.3
Note: The enthalpy of formation of an element in its standard state is
defined as zero.
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