Find AH, q, w, and AE for the freezing of water at -47.80 °C. The specific...

Question

Question

Answer 1

Answer #1

q = 2.087 J/g.^oC * {0 - (-47.8)} ^oC + (333.6 J/g) = 433.36 J/g

Now, $\Delta$ H = 433.36 J/g

Now, w = -P. $\Delta$ V = -R. $\Delta$ T = -8.314 J/mol.K * 47.8 K = -8.314 J/18 g * 47.8 = -22.08 J/g

Finally, $\Delta$ E = $\Delta$ H + w = 433.36 J/g + (-22.08 J/g) = 411.28 J/g

Answer 2

Similar Homework Help Questions

A total of 619 cal of heat is added to 5.00 g of ice at −20.0...

A total of 619 cal of heat is added to 5.00 g of ice at −20.0 °C. What is the final temperature of the water? Specific heat of ?2?(?) 2.087 J/(g⋅°C) Specific heat of ?2?(?) 4.184 J/(g⋅°C) Heat of fusion for ?2? 333.6 J/g
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 75.0 g of H2O(s) at –22.0...

At 1 atm, how much energy is required to heat 75.0 g of H2O(s) at –22.0 °C to H2O(g) at 145.0 °C? Helpful constants can be found here. 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 (steam) 2.000 J/(g·°C) *...

For a process at constant pressure. AE = q and w = 0 AE = w and q = 0. AE=AH AH = 0 Submit Request Answer

For a process at constant pressure. AE = q and w = 0 AE = w and q = 0. AE=AH AH = 0 Submit Request Answer
At 1 atm, how much energy is required to heat 81.0 g of H2O(s) at –20.0...

At 1 atm, how much energy is required to heat 81.0 g of H2O(s) at –20.0 °C to H2O(g) at 149.0 °C? Helpful constants can be found here. These are the helpful constants: 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...
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...

Calculate y, w, AE, and AH, when 299 g of water evaporates at 1.00 atm and...

Calculate y, w, AE, and AH, when 299 g of water evaporates at 1.00 atm and 100.0 °C. The heat of vaporization of water is 40.7 kJ/mol. AH =
1. At 1 atm, how much energy is required to heat 35.0 g H2O(s) at −10.0...

1. At 1 atm, how much energy is required to heat 35.0 g H2O(s) at −10.0 ∘C to H2O(g) at 137.0 ∘C? Use the heat transfer constants found in this 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 (steam) 2.000...
At 1 atm, how much energy is required to heat 73.0 g H2O(s)73.0 g H2O(s) at...

At 1 atm, how much energy is required to heat 73.0 g H2O(s)73.0 g H2O(s) at −14.0 ∘C−14.0 ∘C to H2O(g)H2O(g) at 159.0 ∘C?159.0 ∘C? Use the heat transfer constants found in this table. Heat-transfer constants for H2O at 1 atm 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)...

Please show your work! 6. (2 points) You are given 400 g of coffee (same specific heat as water) at 95.0°C (too hot to S...

Please show your work! 6. (2 points) You are given 400 g of coffee (same specific heat as water) at 95.0°C (too hot to SS drink). How much ice (at 0.0°C) must be added to your coffee in order to cool it to 50.0°C? Neglect heat content of the cup and heat exchanges with the surroundings. Latent heat of fusion of ice is 3.33x10 J/kg: Specific heat of ice is 2100 J/(kgx°C). You must know the specific heat of water....