Question

ID: 10. Identify the place which has the highest boiling point of water, a Death Valley, 282 feet below sea level b. A pressurized passenger jet, 39,000 feet C. Panama City, Florida, sea level d. Mt. Everest, 29,035 feet c. Denver, Colorado, 5,280 feet d. Minha City, Florcnger jet. c. Der Everest, 29 onda, sea le 39,000 feet 11. The heat of vaporization of water at 100°C is 40.66 kJ/mol Calculate the quantity of heat that is absorbed released when 6.00 g of steam condenses to liquid water at 100°C a. 13.5 J of heat are absorbed. b. 13.5 J of heat are released. C. 122 kJ of heat are absorbed. d. 122 kJ of heat are released. c. 244 kJ of heat are released The fluorocarbon C,C1,F3 has a normal boiling point of 47.6°C. The specific heats of C,C1F,C) and C ClsF3(8) are 0.91 J/gK and 0.67 J/gK, respectively. The heat of vaporization of the compound is 27.49 kJ/mol. The heat required to convert 50.0 g of the compound from the liquid at 10.0 C to the gas at 65.0°C is a. 8.46 b. 1454 c. 29.78 d. 2301 e. 9.63 Short Answer 1. Why do 0, F and N, when bonded to H, form such strong intermolecular attractions to neighboring molecules? Make sure to be specific 2. Why does the temperature of a substance stay constant during a phase change such as vaporization? 3. Define boiling point of a liquid. kl. 4. The enthalpy change for converting 1.00 mol of ice at -25.0°C to water at 60.0°C is The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H20, AH 6.01 kJ/mol, and AH -40.67 kJ/mol.

Answer 1

Ans 10

Option A is the correct answer

Atmospheric pressure increases with decreasing above sea level or increasing below sea level and vice versa

Boiling point temperature increases with increasing atmospheric pressure.

Higher the depth below sea level, higher the atmospheric pressure and higher the boiling point temperature.

Higher the elevation above sea level, lower the atmospheric pressure and lower the boiling point temperature.