100.0 g of ice at -15.0°C become steam at 110°C. Using the data reported in the...
100.0 g of ice at -15.0°C become steam at 110°C. Using the data reported in the tables, calculate the amount of heat necessary for the process to occur at standard pressure. Draw the behavior of heat versus temperature. For full credit, report on the plot all the necessary information.
Specific Heat Capacities (J/(g*K))
H2O (s): 2.060
H2O (l), 25°C: 4.184
H2O (g), 100°C: 2.040
Change in Enthalpy of H2O
Fusion: 333.5 J/g
Vaporization: 2260 J/g
Homework Answers
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100.0 g of ice at -15.0°C become steam at 110°C. Using the data
reported in the...
Exercise #11 (65 points) Specific Heat 100.0 g of ice at -15.0°C become steam at 110°C...
Exercise #11 (65 points) Specific Heat 100.0 g of ice at -15.0°C become steam at 110°C Сараcity Using the data reported in the tables, calculate the (J-g1 K1) amount of heat necessary for the process to occur H2O (s) 2.060 at standard pressure. (50 points) Draw the H2О (1), 25°C 4.184 behavior of heat versus temperature. (15 points) 2.040 H2O (g), 100°C For full credit, report on the plot all the necessary information Н2О 333.5 J/g fus H 2260 J/g...
How much heat is released when 105 g of steam at 100.0°C is cooled to ice...
How much heat is released when 105 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). A)347 kJ B)54.8 kJ C)319 kJ D)273 kJ
How much heat (in kJ) is released when 125.0 g of steam at 100.0°C is cooled...
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).
6) There is 15.0 g of ice at 0.0C. How many grams of water at 50.0C must be added to the ice to melt all the ice an...
6) There is 15.0 g of ice at 0.0C. How many grams of water at 50.0C must be added to the ice to melt all the ice and keep the temperature of the mixture at 0.OC? H2O(s)= 2.06J/gc Specific heat: H2O(0) = (4.18 J/g C) H20 heat of vaporization=2260 J/g H2O(g)=(2.03 J/g C) H2O heat of fusion=333 J/g b)25 8 c)23.98 d)7. 58 )0.428
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
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.
How much heat is required to convert 15.0 g of ice at -11.0 °C to steam at 100.0 °C?
How much heat is required to convert 15.0 g of ice at -11.0 °C to steam at 100.0 °C? Express your answer in (a)joules, (b)calories, and (c)Btu.
You add 100.0 g of water at 51.0 °C to 100.0 g of ice at 0.00...
You add 100.0 g of water at 51.0 °C to 100.0 g of ice at 0.00 °C. Some of the ice melts and cools the water to 0.00 °C. When the ice and water mixture reaches thermal equilibrium at 0 °C, how much ice has melted? (The specific heat capacity of liquid water is 4.184 J/g · K. The enthalpy of fusion of ice at 0 °C is 333 J/g.) Mass of ice = References Use the References to access...
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed...
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed in 90.08 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 J K^-1 mol^-1 and 75.3 J K^-1 mol^-1, respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy = ______J/K
To treat a burn on his hand, a person decides to place an ice cube on...
To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 19.2 g, and its initial temperature is −11.2 ∘C. The water resulting from the melted ice reaches the temperature of his skin, 30.1 ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this...
At 1 atm, how much energy is required to heat 43.0 g H2O(s)43.0 g H2O(s) at...
At 1 atm, how much energy is required to heat 43.0 g H2O(s)43.0 g H2O(s) at −14.0 ∘C−14.0 ∘C to H2O(g)H2O(g) at 121.0 ∘C?121.0 ∘C? Use the heat transfer constants found in this table. Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O...
Exercise #11 (65 points) Specific Heat 100.0 g of ice at -15.0°C become steam at 110°C Сараcity Using the data reported in the tables, calculate the (J-g1 K1) amount of heat necessary for the process to occur H2O (s) 2.060 at standard pressure. (50 points) Draw the H2О (1), 25°C 4.184 behavior of heat versus temperature. (15 points) 2.040 H2O (g), 100°C For full credit, report on the plot all the necessary information Н2О 333.5 J/g fus H 2260 J/g...
6) There is 15.0 g of ice at 0.0C. How many grams of water at 50.0C must be added to the ice to melt all the ice and keep the temperature of the mixture at 0.OC? H2O(s)= 2.06J/gc Specific heat: H2O(0) = (4.18 J/g C) H20 heat of vaporization=2260 J/g H2O(g)=(2.03 J/g C) H2O heat of fusion=333 J/g b)25 8 c)23.98 d)7. 58 )0.428
You add 100.0 g of water at 51.0 °C to 100.0 g of ice at 0.00 °C. Some of the ice melts and cools the water to 0.00 °C. When the ice and water mixture reaches thermal equilibrium at 0 °C, how much ice has melted? (The specific heat capacity of liquid water is 4.184 J/g · K. The enthalpy of fusion of ice at 0 °C is 333 J/g.) Mass of ice = References Use the References to access...
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