Heat of Fusion and Heat of Vaporization Worksheet Q= mH, Q= mH, Q= mH. Q = heat energy (3) m = mass (g) H = heat of fusion (3/g) H, = heat of vaporization (3/g) H. = heat of condensation (3/9) 1. Calculate the heat energy required, in joules, to melt 5.00 x 10 grams of ice which is at 0.0°C. The heat of fusion of ice is 333.6 J/g. ice (0.0°C) - water (0.0°C) 2. Calculate the heat released when 2.00 x 10 grams of steam at 100°C condenses to form water at 100 C. The heat of condensation of steam is 2258 J/g. steam (100°C) water (100°C) 3. Liquid ammonia is a common refrigerant because it absorbs so much heat energy when it turns from the liquid to a gas. The heat of vaporization of liquid ammonia is 1374 3/g. Calculate the heat needed to turn 454 grams of liquid ammonia at its boiling point to ammonia gas at the same temperature. NH3(() - NH3(g)

Heat of Fusion and Heat of Vaporization Worksheet Q= mH, Q= mH, Q= mH. Q = heat energy (3) m = mass (g) H = heat of fusion (3/g) H, = heat of vaporization (3/g) H. = heat of condensation (3/9) 1. Calculate the heat energy required, in joules, to melt 5.00 x 10 grams of ice which is at 0.0°C. The heat of fusion of ice is 333.6 J/g. ice (0.0°C) - water (0.0°C) 2. Calculate the heat released when 2.00 x 10 grams of steam at 100°C condenses to form water at 100 C. The heat of condensation of steam is 2258 J/g. steam (100°C) water (100°C) 3. Liquid ammonia is a common refrigerant because it absorbs so much heat energy when it turns from the liquid to a gas. The heat of vaporization of liquid ammonia is 1374 3/g. Calculate the heat needed to turn 454 grams of liquid ammonia at its boiling point to ammonia gas at the same temperature. NH3(() - NH3(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How much ice in grams would have to melt to lower the temperature of 342 mLmL of water from 35 ∘C∘C to 0 ∘C∘C? (Assume that the density of water is 1.0 g/mLg/mL.)
Given that for liquid water, AH(fusion)=334J/g, how much is needed to melt approximately 34.2 grams of ice?
6. A substance has the following properties; Boiling Point = 120°C, Freezing Point = -20°C, specific heat as a gas, liquid and solid, 0.8 cal/g-C°, 3 cal/g-C° and 2 cal/g-C°, respectively. Heat of fusion=200 cal/g and heat of vaporization=800 cal/g. How much heat must be added in changing 100g of this substance from -40°C to 180°C?
mFe = 49.28g, with a MP of 1538oC. Given ∆Hfus = 276J/g, how much heat is required to melt Fe?
What is the enthalpy (in J) required to melt a 4.77g block of Ice? H fusion= 6.00) kJ/mol
How many joules of energy must be removed from 152 g of water at 18.5 °C to form ice at 0 °C?
If we start with 10g of ice at -5°C and heat it until we have liquid water at 45°C, how much heat energy will be needed (kJ)? The specific heat of ice is 2.03J/g°C and the specific heat of liquid water is 4.18J/g°C. ΔHfusion is 334 J/g.
4. Calculate the amount of energy absorbed when 5g ice @ 0°C melts to water at 0°C. Did a phase change occur? If so, which one? Is this endothermic or exothermic?
You pour 84 mL of 1.5 M HNO3 and 284 mL of 0.50 M KOH over 50 g ice. The solutions and the ice were both initially at 0C. How much ice melts? Assume the heat of neutralization is -57.3 kJ/mol.
How many kJ of energy are needed to change 19.3 g of ice at 0.00 °C to water at 20.66 °C? Use a heat of fusion of ice of 333.6 J/g and a specific heat of water of 4.184 J/gºC. Give the answer with the correct number of sig figs.
How many joules of energy must be removed from 177 g of water at 16.3 °C to form ice at 0 °C?
3. Calculate the heat required to increase the temperature of 630 grams of ice from -2℃ to 23℃ and turn it to steam with temperature of 124℃. The specific heat of ice is 2.108 J/(g∙℃).