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Concept explainers
Interpretation:
Energy needed for conversion of
Concept Introduction:
Heat required by
Heat of fusion is amount of heat required to convert solid to liquid. Every substance has different heat of fusion. Heat of fusion for ice is
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Answer to Problem 56AE
Energy needed for conversion of
Explanation of Solution
The formula to calculate energy of ice is as follows:
Here,
Substitute
The formula to calculate energy needed for conversion of ice to water is as follows:
Here,
Substitute
The formula to calculate energy of water is as follows:
Here,
Substitute
Therefore, total energy needed for conversion of ice to water is as follows:
Substitute
Hence, energy needed for conversion of
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Chapter 13 Solutions
EBK FOUNDATIONS OF COLLEGE CHEMISTRY
- Explain why 15 g of steam at 100C melts more ice than 15 g of liquid water at 100C.arrow_forwardCalculate the quantity of heating required to convert the water in four ice cubes (60.1 g each) from H2O(s) at 0 °C to H2O(g) at 100. °C. The enthalpy of fusion of ice is 333 J/g and the enthalpy of vaporization of liquid water is 2260 J/g.arrow_forwardThe vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.arrow_forward
- Calculate the amount of heat that must be absorbed by 24.0 g of ice (-15°C) to convert it to water at 50°C. The specific heat of ice and water is 2.09 and 4.18 J/g-°C, respectively. The heat of fusion and heat of vaporization is 334 and 2260 J/g, respectively.arrow_forwardAn ice cube at 0.00 °C with a mass of 8.64g is placed into 85.0g of water at 45°C. If no heat is lost to the surroundings, what is the final temperature of the water sample after all the ice is melted. (The specific heat of water is 4.184J/g°C, the ∆Hfus = 6.02kJ/mol)arrow_forwardCalculate the energy in the form of heat (in kJ) required to change 76.9 g of liquid water at 25.2 °C to ice at –15.2 °C. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: ice = 2.06 J/g⋅K, liquid water = 4.184 J/g⋅K)arrow_forward
- What is the amount of heat in kilojoules required to convert 447.0 g of ice at −15.2°C to liquid water at 35.6°C? The specific heat of ice is 2.03 J/g·°C.The molar heat of fusion of ice is 6010 J/mol. The specific heat of water is 4.184 J/g·°C.arrow_forwardWhat quantity of heat (in kJ) would be required to convert 21.0 g of ice to water at 0.00 °C? (AHfus = 6.01 kJ/mol for water)arrow_forwardat 100.0C the molar heat of vaporization of water is 40.67KJ/mol. at 25.0C approximately room temperature, the molar heat of vaporization of water is 44.0KJ/mol. during a strenuous work out, an athlete generates 2010KJ of heat energy. what mass of water would have to evaporate from the athletes skin to dissipate 2010KJ of heat? in gramsarrow_forward
- How much heat is released ( in J) when 54.0 g of water at 10.0 °C is cooled to form ice at -10.0 °C? Molar mass of H2O = 18.0 g/molSpecific heat capacity of H2O(s) = 2.09 J/g. °CSpecific heat capacity of H2O(l) = 4.18 J/g. °C∆Hfus= 6.02 kJ/molBoiling point of water is 100.0°CFreezing point of water is 0.0 °Carrow_forwardThe enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is ________ kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol.arrow_forwardA 22.5-g sample of ice at-10.7°C is mixed with 103.0 g of water at 80.0°C. Calculate the final temperature of the mixture, assuming no heat loss to the surroundings. The heat capacities of H20(s) and H2O(1) are 2.03 J/g.°C and 4.18 J/g.°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol. [References] Temperature = °C Submit Answer Try Another Version 10 item attempts remaining Visited 11: 12/6 33°F archarrow_forward
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