y is 13.6 genn from the gas to the s 0.140 g K and its heat of fusion is 11.4 J/
ID: 1010288 • Letter: Y
Question
y is 13.6 genn from the gas to the s 0.140 g K and its heat of fusion is 11.4 J/g.) by 1.88 L. What is t ed to raise 22. What of energy, in joules, is requir the temperature from room temperature the gas 25.0 C, to its melting point, 231.9 oc, and Enthalpy Changes the tin at that (The specific heat capacity Ex of tin is temperature fusion of this (See Section 5-5 and J/g K, and the heat of metal is 59.2 J/g.) 33 Nitrogen monoxi in a wide range 23. Ethanol, C2HsoH, boils at 78.29 °C. How much energy, oxygen to give b f 1.000 kg. n joules, is required to raise the temperature o to of ethanol from 20.0 oC to the boiling point and then 2 NO (g) O2 change the liquid to vapor at that temperature? (The specific heat capacity of liquid ethanol is 2.44 Jg K Is this reaction and its enthalpy of vaporization is 8 Jlg.) enthalpy chan 24. A 25.0 ml sample of benzene at 19.9 °C was cooled to pletely to NO its melting point, 5.5 oC, and then frozen. How much 34. Calcium carb energy was given off as heat in this process (The of CaO with density of benzene is 0.80 g/mL, its specific heat capac- ity is 1.74 J/g K, and its heat of fusion is 127 Jlg.) carbide is th CaO(s) Heat, Work, and Internal Energy (See Section 5-4 and Example 5.5.) 25. As a gas cools, it is compressed from 2.50 L to 1.25 L Is this rea under a constant pressure of 1.0 x 105 Pa. Calculate enthalpy the work (in required to compress the gas. with an eExplanation / Answer
Total energy = energy required to increased temperature + energy required to convert liquid to vapor
Mass of ethanol = 1.0 kg = 1000 g
Q = mc(T2-T1) + dH vap * m
Q= 1000 * 2.44 (78.29- 20.00) + 1000*855
= 142227.6 J+ 855000 J
= 997227.6 J
= 997.2 KJ
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