Calculate the heat required to convert 18.6 g of propyl alcohol, C3H8O, from a solid at -150°C into the gaseous state at 113°C. The normal melting and boiling points of this substance are -127°C and 97°C, respectively. The heat of fusion is 86.2 J/g, and the heat of vaporization is 694 J/g. The specific heats of the solid, liquid and gaseous states are, respectively, 2.36, 2.83 and 1.76 J/g/K.

Calculate the heat required to convert 18.6 g of propyl alcohol, C3H8O, from a solid at -150°C into the gaseous state at 113°C. The normal melting and boiling points of this substance are -127°C and 97°C, respectively. The heat of fusion is 86.2 J/g, and the heat of vaporization is 694 J/g. The specific heats of the solid, liquid and gaseous states are, respectively, 2.36, 2.83 and 1.76 J/g/K.

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

The density of liquid oxygen at its boiling point is 1.14 kg/Lkg/L , and its heat of vaporization is 213 kJ/kgkJ/kg . How much energy in joules would be absorbed by 3.0 LL of liquid oxygen as it vaporized? Express your answer to two significant figures and include the appropriate units. ------ Water's heat of fusion is 80. cal/gcal/g , and its specific heat is 1.0calg⋅∘Ccalg⋅∘C . Some velomobile seats have been designed to hold ice packs inside their cushions. If you started a ride with ice packs that held 1300 gg of frozen water at 0 ∘C∘C , and the temperature of the water at the end of the ride was 32 ∘C∘C , how many calories of heat energy were absorbed? Express your answer to two significant figures and include the appropriate units. ---- Water's heat of fusion is 80. cal/gcal/g , its specific heat is 1.0calg⋅∘Ccalg⋅∘C, and its heat of vaporization is 540 cal/gcal/g . A canister is filled with 330 gg of ice and 100. gg of liquid water, both at 0 ∘C∘C . The canister is placed…
What amount of heat (in kJ) is required to convert 14.7 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g. °C; specific heat capacity of gas = 0.932 J/g °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3 °C)
Ethanol (C2H5OH) melts at -114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/gK and 2.3 J/gK, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135°C to liquid ethanol at -40°C?
Converting a 5.00 g sample of liquid cyclohexane (C6H₁2) at 30.7 °C to vapor at 140.7 °C requires kJ of heat. molar mass = 84.16 g/mol melting point = 6.5 °C boiling point = 80.7 °C AHfus = 2.68 kJ/mol AHvap = 32.0 kJ/mol Csolid 1.2 J/g °C Cliquid 2.8 J/g °C Cgas = 0.90 J/g °C
The specific heat of liquid thallium, TI, is 0.13 J/g C. The heat of fusion of thallium is 4.29 kJ/mol. The heat of vaporization of thallium is 162.5 kJ/mol. How much heat is required to change 10.0 g of solid thalium at 304 degrees C to vapor at 1457 degrees C? The melting point of thallium is 304 degrees C. The boiling point of thallium is 1457 degrees C. 21 J 3.2x 10 3 J 8.2x 10 1 33 J 2.7x 104 J 86 J 1.9x 10 2) 9.7x 103J Previous Next
Calculate the heat, in kilocalories, that is absorbed if 139 g of ice at 0.0 ∘C is placed in an ice bag, melts, and warms to body temperature of 37.0 ∘C. The heat of fusion for water is 80. cal/g, or 334 J/g. The specific heat for water is 1.00 cal/g∘C, or 4.184 J/g∘C.
11. Based on the heating graph shown in the figure for a substance, X, at constant pressure, Energy transferred a) Which has the largest specific heat capacity, X(s), X(e), or X(g)? b) Which is smaller, the heat of fusion or the heat of vaporization? c) What is the algebraic sign of the enthalpy of vaporization at the boiling point? Temperature, 7T +
How much energy is needed to convert 59.5 grams of ice at 0.00 celsius to water at 60.9 celsius? specific heat(ice) = 2.10 J/g specific heat (water) 4.18 J/g heat of fusion= 6.02 kJ/mol heat of vaporization= 40.6 kJ/mol
Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °C
Ethanol (C2H5OH) melts at -114 oC and boils at 78 oC. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol the specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat is required to convert 20.18 g of ethanol at -220 oC to the vapor phase at 78 oC? (Give your answer in unit of kilojoules)
Ethanol (C2H5OH) melts at -114 oC and boils at 78 oC. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol the specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat is required to convert 31.55 g of ethanol at -200 oC to the vapor phase at 78 oC? (Give your answer in unit of kilojoules)
What amount of heat (in kJ) is required to convert 10.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g. °C; specific heat capacity of gas = 0.932 J/g⋅ °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3 °C)