The molar heat of fusion of lithium metal is 3.00 kJ/mol, whereas its heat of vaporization is 147 kJ/mol.  a. What quantity of heat would be needed to melt 1.00 g lithium at its normal melting point? b. What quantity of heat would be needed to vaporize 1.00 g lithium at its normal boiling point? c. What quantity of heat would be evolved if 1.00 g lithium vapor condensed at its normal boiling point?

[Review Topics] The molar heats of fusion and vaporization for silver are 11.3 kJ/mol and 250.0 kJ/mol, respectively. Silver's normal melting point is 962 °C, and its normal boiling point is 2212 °C. a. What quantity of heat is required to melt 15.0 g of silver at 962 °C? kj b. What quantity of heat is liberated when 4.34 g of silver vapor condenses at 2212 °C? kj Submit Answer In progress Retry Entire Group 9 more group attempts remaining Show Hint [References] Previous Next Save and Exit

carbon disulfide Cs2 has a heat of vaporization of 29,200 J/mol. at 268 K it has a vapor pressure of 1.0 X 10^2 mmHg. what is its vapor pressure at 301 K

Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1,809 K), given that ΔHfus = 13.80 kJ/mol. A.   27.6 kJ B.   25,000 kJ C.   27,600 kJ D.   27,600 J E.   494 kJ

1. Calculate the amount of heat (in kJ) released when converting 150.2 g of water to ice at -23 degrees Celsius.    2. A closed vessel of volume 10.0 L initially contains 1.303 g of water and no water vapor. Please calculate the mass of liquid water remaining once the system reaches equilibrium at 30 degrees Celsius. The vapor pressure of water at that temperature is equal to 0.0418 atm.   3. A person drinks four glasses of cold water (5 degrees C) every day. The volume of each glass is 195. mL. How much heat (in kJ) does the body have to supply to raise the temperature of the water to 37 degrees C (body temperature)?   4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O­2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction:                 N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l)   5. Consider the following chemical equation. CH4(g) + 2O2(g) à CO2(g) + 2H2O(l)                 Using the values in the table, calculate…

1. Freon-12 (CCl2F2) is banned as a refrigerant because it is harmful to the ozone. a. Sketch the phase diagram of CCl2F2 using the physical constants below Normal boiling point = -29.8 °C Normal melting point = -158 °C Critical temperature = 112 °C Critical pressure = 40.8 atm Triple point (2.42 ×10-6 atm, -157 °C) b. Calculate the heat required to bring 10.0g CCl2F2 from -29.8 °C as a liquid to the gas phase at 10.0 °C. (molar mass 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K AHvap = 20.1 kJ/mol AHfus = 4.14 kJ/mol

Aluminum has a cubic closest packed structure as a solid. Assuming that aluminum has an atomic radius of 143 pm, calculate the density of solid aluminum. g/cm³

A chemist has two beakers, One beaker contains nonpolar liquid A. The other beaker contains polar liquid B. Which statement is most likely true? O Liquid A has a lower vapor pressure than liquid B. O Liquid A has a higher normal boiling point than liquid B. O Liquid A has stronger intermolecular attractions than liquid B. The heat of vaporization for liquid A is lower than that for liquid B.