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.
ID: 10. Identify the place which has the highest boiling point of water, a Death Valley,...
11. The following would be required for calculations of heat flow in which of the heating curve steps ? Molar heat of vaporization of water (AH vap = 40.7 kJ/mol) Specific heat of ice (Cice = 2.09 J/g °C) Molar heat of fusion of water (AH fus = 6.02 kJ/mol) Specific heat of water (C H20 = 4.18 J/g °C) Specific heat of steam(C steam = 2.01 J/g °C) Heating Curve for Water Degrees Celsius -50+ 0 400 800 1200...
4 pts Question 15 Identify the place which has the highest boiling point of water. A) Death Valley, 282 feet below sea level B) a pressurized passenger jet, 35,000 feet C) New Orleans, sea level D) Mt. Everest, 29,035 feet OD OB ос ОА 4 pts Question 16
The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g⋅K and 0.67 J/g⋅K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat required to convert 45.5 g of C2Cl3F3 from a liquid at 14.10 ∘C to a gas at 78.40 ∘C. Express your answer using two significant figures.
if u can show how u do each one, that would be amazing! How much heat is required to convert 90 g of ice at - 40.0°C into water at 60.0°C? The specific heats (Cs) of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H0 AH A) 60.1 kJ = 6.01 kJ/mol, and AH B) 18.8 kJ -40.67 kJ/mol. C) 45.1 kJ D) 37.6 kJ E) 30.5 kJ 11. What is correct for a...
Calculate the heat required in Joules to convert 18.0 grams of water ice at a temperature of -20° C to liquid water at the normal boiling point of water. Given: -specific heat of ice = 2.09 J/g°C -specific heat of liquid water = 4.184 J/g°C -specific heat of water vapor = 2.03 J/g°C -molar heat of fusion of water = 6.02 kJ/mol -molar heat of vaporization of water = 40.7 kJ/mol
The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed/released when 5.00 g of steam condenses to liquid water at 100°C. 147 kJ of heat are absorbed. 147 kJ of heat are released. 11.3 kJ of heat are absorbed 11.3 kJ of heat are released.
The heat of vaporization of water at 100°C is 46.06 kJ/mol. Calculate the quantity of heat that is absorbed/released when 90.0 g of steam condenses to liquid water at 100°C. 203 kJ of heat are absorbed. 20.3 kJ of heat are released. 230.3 kJ of heat are released. 203.3 kJ of heat are released.
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.
Enter your answer in the provided box. How much heat (in kJ) is needed to convert 916 g of ice at -10.0°C to steam at 126.0°C? (The specific heats of ice, water, and steam are 2.03 J/g . oC, 4.184 J/g . oC, and 1.99 J/g , oC, respectively. The heat of fusion of water is 6.01 kJ/mol, the heat of vaporization is 40.79 k.J/mol.) k.J
How much heat (in kJ) is released when 125.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).