7:00 AM Wed Feb 1 Question 17 of 26 Ice cubes at 0 °C with a total mass of 435 g are put in a microwave oven and heated with 750. W (750. J/s) of energy for 6.00 minutes. What is the final temperature of the water from the melted ice in °C? Assume all of the microwave energy is absorbed by the ice/water and no heat loss by the ice/water. The enthalpy of fusion for ice is 6.02 kJ/mol and the specific heat capacity for water is 4.184 J/g °C. Tap here or pull up for additional resources 1 4 7 8 +/- I 25 . 36 °C 9 O

7:00 AM Wed Feb 1 Question 17 of 26 Ice cubes at 0 °C with a total mass of 435 g are put in a microwave oven and heated with 750. W (750. J/s) of energy for 6.00 minutes. What is the final temperature of the water from the melted ice in °C? Assume all of the microwave energy is absorbed by the ice/water and no heat loss by the ice/water. The enthalpy of fusion for ice is 6.02 kJ/mol and the specific heat capacity for water is 4.184 J/g °C. Tap here or pull up for additional resources 1 4 7 8 +/- I 25 . 36 °C 9 O

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...

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Draw the heating curve for ice at -30.0 °C to steam at 130.0 °C and label the phases on the lines in the heating curve. Show this in your work and upload the file in the last question. In the box below, calculate the enthalpy ( in kJ)for converting 50.0 g of ice at -15.0 °C to water at 58.4 °C. (Show work below the heating curve). The specific heat of ice = 2.09 J/g-°C The specific heat of water = 4.184 J/g-°C he specific heat of steam = 1.84 J/g-°C ΔHfus for water = 6.01 kJ/mol ΔHvap for water = 40.67 kJ/mol Enter the numerical value in the box. Give 3 sig figs in your answer.
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Suppose you have a perfectly insulated container holding 2.00 kg of liquid water at a temperature of 20.0°C. You also have a large supply of ice cubes which are stored at a temperature of-20.0°C. (a) What is the maximum mass of ice you can add to the water so that all of the ice melts? Assume no heat is lost to the environment. (b) Suppose you add twice the mass of ice that you found in part a. How much solid ice will remain once thermal equilibrium is reached?
Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro
What amount of thermal energy (in kJ) is required to convert 221 g of ice at -16 °C completely to water vapour at 214 °C? The melting point of water is 0 °C and its normal boiling point is 100 °C. The heat of fusion of water is 6.02 kJ mol-¹ The heat of vaporization of water at its normal boiling point is 40.7 kJ mol-¹ The specific heat capacity of ice is 2.09 J g-¹ °C-¹ The specific heat capacity of liquid water is 4.18 J g-¹ °C-¹ The specific heat capacity of water vapour is 2.01 Jg¹¹ °C-¹ Answer:
What amount of heat (in kJ) is required to convert 15.5 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)
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Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T;, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/(mol·K) Tf = heat capacity of H,O(l) 75.3 J/(mol-K) enthalpy of fusion of H,O 6.01 kJ/mol
Sulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at −73.0 ° C and boils at −10.0 ° C. Its Δ H o fus is 8.619 kJ/mol, and its Δ H o vap is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g · K and 0.622 J/g · K, respectively. How much heat is required to convert 7.750 kg of solid SO2 at the melting point to a gas at 60.0 ° C?