A 124.0 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 \deg C to 147.6 \deg C. ( heat capacity of liquid = 1.62 J/g. \deg C; heat capacity of gas = 1.04 J/g. \deg C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 \deg C) How much energy (in kJ) is absorbed/released to condense the gas?

A 124.0 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 \deg C to 147.6 \deg C. ( heat capacity of liquid = 1.62 J/g. \deg C; heat capacity of gas = 1.04 J/g. \deg C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 \deg C) How much energy (in kJ) is absorbed/released to condense the gas?

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...

See similar textbooks

Similar questions

4
The following information is given for benzene, CáHá, at 1atm: AHvap(80.1 °C) = 30.7 kJ/mol boiling point 80.1 °C specific heat liquid = KJ 1.74 J/g °C At a pressure of 1 atm, what is AH in kJ for the process of condensing a 47.4 g sample of gaseous benzene at its normal boiling point of 80.1 °C.
A 51.76 g51.76 g sample of a substance is initially at 28.0 °C.28.0 °C. After absorbing 1755 J1755 J of heat, the temperature of the substance is 171.0 °C.171.0 °C. What is the specific heat (?c) of the substance?
What amount of heat is required to convert 10.9 g of an unknown liquid (MM 83.21 g/mol) at 19.2°C to a gas at 93.5 °C? (heat capacity of iquid 1.58 J/g.C; heat capacity of gas 0.932 JIg.°C; AHvap 22.5kJ/mol, Tb= 57.3°C) kJ
Propane gas (C3H6 (g)) is withdrawn from a 100.0 L cylinder at 25.0 oC and is burned at constant pressure in an excess of oxygen. The pressure in the cylinder falls from 2.25 atm to 1.05 atm. The liberated heat is then used to raise the temperature of 65.5 L of water from 25.0 oC to 56.7 oC. What % of the heat of combustion was absorbed by the water (d = 1.00 g/mL)? Specific heat capacity of water = 4.18 J/g/oC Δ Hfo(H2O(l)) = -285.8 kJ/mol, Δ Hfo(O2(g)) = 0 kJ/mol, Δ Hfo(CO2 (g)) = -393.5 kJ/mol Δ Hfo(C3H6 ) = -103.8 kJ/mol
The addition of 105.0 g potassium fluoride to 599.0 mL of water (d = 1.00 g/mL) causes the temperature to rise 3.21 °C. What is the ΔHrxn for KF? (Assume cp = 4.18 J/g oC.)
14. See image below. MM of Al:Os = 101.96 g/mol: 14. Calculate the amount of heat released in the complete combusti on of 8.17 grams of Al to form solid Alz03 at 25°C and 1 atm. AH for Al2O3 = 1676 kJ/mol 4Al) + 30(g) → 2Al:O: (5) 237 kJ O 254 kJ O 203 kJ O 127 kJ
[Relerences] Acetaldehyde, CH; CHO, is a colorless, flammable liquid used in the manufacture of acetic acid, perfumes, and flavors. What is the heat of vaporization of CH3CHO? CH3 CHO(1) → CH3 CHO(g); AH° =? AH;(CH3CHO(1)) = – 191.8 kJ/mol AH;(CH3 CHO(g)) = - 166.1 kJ/mol Heat of vaporization = kJ Submit Answer Try Another Version 6 item attempts remaining Previc e to search
Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? qlost = m·Hv + m·Cp·ΔT.
From 25.0°C to 94.5°C, 75.1 grams of ethanol are heated. What was the energy requirement in joules?H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. cp (liquid) ethanol 2.46 J/g°C, cp (gas) ethanol 1.43 J/g°C, and cp (solid) ethanol 2.42 J/g°C are the specific temperatures for the three phases of ethanol. Ethanol has a molecular weight of 46. The melting point of ethanol is -114.1 °C and the boiling point is 78.4 °C.
Calculate the amount of heat (in kJ) required to raise the temperature of a 86.0 g sample of ethanol from 198.0 K to 300.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. 60.0 kJ 21.2 kJ 11.9 kJ 75.6 kJ 28.4 kJ
As a substance is subjected to pressure and/or temperature changes, it may undergo condensation, deposition, freezing, melting, sublimation, or vaporization. (a) Consider the phase diagram shown below and state the cha nges that take place upon going from points A to B to C to D. (b) Is the transition from C to D exothermic or endothermic?