KJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK and 1.84 J/gK The enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is respectively. For H2O, AHfus = 6.01 kJ/mol, and AHvap = 40.67 kJ/mol. O 9.88 O 3870 O 6.16 O 12.28

How much heat is released when 105 g of steam at 100.0 C is cooled to ice at -­15.0 C? The enthalpyof vaporization of water is 40.67 kj/mol, the enthalpy of fusion for water is 6.01 kj/mol, the specific heatcapacity of liquid water is 4.18 J/g C and the specific heat capacity of ice is 2.02 J/g C.(q heating = m x C x ΔT, q phase change = ΔH vap x n)

A total of 537 cal of heat is added to 5.00 g of ice at -20.0 °C. What is the final temperature of the water? Tfinal = °C Specific heat of H₂O(s) Specific heat of H₂O(l) Heat of fusion for H₂O 2 2.087 J/(g. °C) 4.184 J/(g. °C) 333.6 J/g

kJ. The specific heats of ice, water, and The enthalpy change for converting 1.00 mol of ice at -50.0 °C to water at 60.0°C is steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g - K, respectively. For H₂O, A Hfus = 6.01kJ/mol, and AHvap = 40.67 kJ/mol. 6401 12.28 12.41 6.37 8.64

1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at -20C to convert it to liquid water at 60.0C. Given: Specific heat (ice) = 2.1 J/g.C Specific heat (water) = 4.18 J/g-C Hfus = 6.0 kJ/mol or 334 J/g

Calculate the enthalpy change upon converting 45g of steam at 150 C to ice at -30 C under a constant pressure of 1 atm. The specific heats of ice, liquid water, and steam are 2.03, 4.18, and 1.84 J/g-K, respectively.

How much heat must be added to 100 g of ice at -5°C to turn it into 60 grams of water and 40 grams of steam, both at 100°C? Cp H2O = 75.7 J/mol-K, Cp Ice = 37.7 J/mol-K, Cp Steam = 35.1 J/mol-K, ΔHfus = 6.01 kJ/mol, ΔHvap = 40.7 kJ/mol