A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g...
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C.
a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C.
b) What is the total heat needed to melt the 75g of ice?
c) What is the total amount of heat required to raise the temperatur of the water formed to 60 degrees C?
d) What is the total amount of heat in kJ needed to melt 75g of ice and heat the resulting water to a final temperature of 60 degrees C
e)What would be the toal mass of butane, C4H10 that would need to be combusted in order to melt 75g of ice at 0 degrees C and heat the resulting water to a final temperature of 60 degrees C? 2C4H10+13O2 8CO2+ 10H2O delta change H=5745kJ
Please show supporting evidence.
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C.
a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C.
b) What is the total heat needed to melt the 75g of ice?
c) What is the total amount of heat required to raise the temperatur of the water formed to 60 degrees C?
d) What is the total amount of heat in kJ needed to melt 75g of ice and heat the resulting water to a final temperature of 60 degrees C
e)What would be the toal mass of butane, C4H10 that would need to be combusted in order to melt 75g of ice at 0 degrees C and heat the resulting water to a final temperature of 60 degrees C? 2C4H10+13O2 8CO2+ 10H2O delta change H=5745kJ
Please show supporting evidence.
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C.
a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C.
b) What is the total heat needed to melt the 75g of ice?
c) What is the total amount of heat required to raise the temperatur of the water formed to 60 degrees C?
d) What is the total amount of heat in kJ needed to melt 75g of ice and heat the resulting water to a final temperature of 60 degrees C
e)What would be the toal mass of butane, C4H10 that would need to be combusted in order to melt 75g of ice at 0 degrees C and heat the resulting water to a final temperature of 60 degrees C? 2C4H10+13O2 8CO2+ 10H2O delta change H=5745kJ
Please show supporting evidence.
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C.
a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C.
b) What is the total heat needed to melt the 75g of ice?
c) What is the total amount of heat required to raise the temperatur of the water formed to 60 degrees C?
d) What is the total amount of heat in kJ needed to melt 75g of ice and heat the resulting water to a final temperature of 60 degrees C
e)What would be the toal mass of butane, C4H10 that would need to be combusted in order to melt 75g of ice at 0 degrees C and heat the resulting water to a final temperature of 60 degrees C? 2C4H10+13O2 8CO2+ 10H2O delta change H=5745kJ
Please show supporting evidence.
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C.
a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C.
b) What is the total heat needed to melt the 75g of ice?
c) What is the total amount of heat required to raise the temperatur of the water formed to 60 degrees C?
d) What is the total amount of heat in kJ needed to melt 75g of ice and heat the resulting water to a final temperature of 60 degrees C
e)What would be the toal mass of butane, C4H10 that would need to be combusted in order to melt 75g of ice at 0 degrees C and heat the resulting water to a final temperature of 60 degrees C? 2C4H10+13O2 8CO2+ 10H2O delta change H=5745kJ
Please show supporting evidence.
Homework Answers
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A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0
g...
what is the final temperature when a 60 g of ice at 0 degrees C. is...
what is the final temperature when a 60 g of ice at 0 degrees C. is added to 200 g of water at 25 degrees C.?
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To cool her 0.200 kg cup of 75.0 C hot chocolate (mostly water), Heidi drops a 29,.97 g ice cube at 0 C into her insulated cup. After the ice cube melts, the temperature of the hot chocolate comes down to 54.8 C. a. How much energy was lost by the hot chocolate? The specific heat capacity of water is 1 cal/g C b. How much energy was gained by the ice cube just to melt to 0 C water?...
Video 2 0°c 2. Ice at his combined with 50.0g of water at 75.0°C. Calculate the...
Video 2 0°c 2. Ice at his combined with 50.0g of water at 75.0°C. Calculate the grams of ice present initially if the entire mixture comes to a final temperature of 25.0°C after the ice melts. Specific heat of water is 4.18 J/gºC, AH, = 334J/g Specific heat of water is 4.18 J/gºC, AH, = 334J/g
A total of 581 cal of heat is added to 5.00g ice at -20 C. What...
A total of 581 cal of heat is added to 5.00g ice at -20 C. What is the final temperature of the ice? Specific heat of H2O (SOLID) = 2.087 Specific heat of H2O (Liquid)= 4.184 Heat of fusion of H2O = 333.6J/g Hint: The total amount of energy needed is equal to the sum of heat needed to warm the ice to 0.0 C, melt the ice and warm the water to its final temperature
A 200 g piece of ice at 0 degrees Celsius is place in 500 g of...
A 200 g piece of ice at 0 degrees Celsius is place in 500 g of water at 20 degrees Celsius. The system is in a container of negligible heat capacity and insulated from its surroundings. a) What is the final equilibrium temperature of the system? b) How much of the ice melts? The latent heat of fusion for water is (333.5 KI/kg). The specific heat of water is 4.18 KI/kg K Useful equations: Q = mlf and Q =...
4. A 100 g block of ice at 0°C is placed in bowl containing 100 g...
4. A 100 g block of ice at 0°C is placed in bowl containing 100 g of water at a temperature of 50°C. Neglecting the energy transferred to the bowl, which statement best describes the flow of heat energy and the final temperature of the mixture when they reach equilibrium? a. b. c. d. e. Heat flows from the ice to the water and the final temperature of the mixture will be 0°C. Heat flows from the water to the...
A 40-g block of ice is cooled to −75°C and is then added to 570 g...
A 40-g block of ice is cooled to −75°C and is then added to 570 g of water in an 80-g copper calorimeter at a temperature of 26°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g · °C...
A 40-g block of ice is cooled to −77°C and is then added to 590 g...
A 40-g block of ice is cooled to −77°C and is then added to 590 g of water in an 80-g copper calorimeter at a temperature of 23°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g · °C...
A 40-g block of ice is cooled to -71°C and is then added to 610 g...
A 40-g block of ice is cooled to -71°C and is then added to 610 g of water in an 80-g copper calorimeter at a temperature of 23°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g·°C = 2,090...
A 200 g ice cube at -20 degrees Celsius is placed in 1.00 kg of water...
A 200 g ice cube at -20 degrees Celsius is placed in 1.00 kg of water at 25 degrees Celsius in a 50 g aluminum calorimeter also at 25 degrees Celsius. A. How much heat does the ice cube absorb as it reaches its melting point? B. How much heat does the ice cube absorb as it melts? C. What is the final tempreature pf the mixture? D. How much heat does the water in the calorimeter lose as it...
Video 2 0°c 2. Ice at his combined with 50.0g of water at 75.0°C. Calculate the grams of ice present initially if the entire mixture comes to a final temperature of 25.0°C after the ice melts. Specific heat of water is 4.18 J/gºC, AH, = 334J/g Specific heat of water is 4.18 J/gºC, AH, = 334J/g
A 200 g piece of ice at 0 degrees Celsius is place in 500 g of water at 20 degrees Celsius. The system is in a container of negligible heat capacity and insulated from its surroundings. a) What is the final equilibrium temperature of the system? b) How much of the ice melts? The latent heat of fusion for water is (333.5 KI/kg). The specific heat of water is 4.18 KI/kg K Useful equations: Q = mlf and Q =...
4. A 100 g block of ice at 0°C is placed in bowl containing 100 g of water at a temperature of 50°C. Neglecting the energy transferred to the bowl, which statement best describes the flow of heat energy and the final temperature of the mixture when they reach equilibrium? a. b. c. d. e. Heat flows from the ice to the water and the final temperature of the mixture will be 0°C. Heat flows from the water to the...
A 40-g block of ice is cooled to -71°C and is then added to 610 g of water in an 80-g copper calorimeter at a temperature of 23°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g·°C = 2,090...
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