The latent heat of vaporization of ethanol is 200 calories/gram. this means that _____.

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a) about 200 calories of heat must be added to 1 gram of ethanol to change its temperature b) about 200 calories of heat must be added to 1 gram of ethanol to convert it from a solid to a liquid c) about 200 calories of heat must be added to 1 gram of ethanol to convert it from a liquid to a gas

How do I figure this one out?

1. How do you figure this out? Learn what the heat of vaporization is:

   http://www.physlink.com/education/askexperts/ae93.cfm

   👤

2. Okay, thank you.

3. a block of aluminum weighing 140. g is cooled from 98.4 c to 62.2 c with the release of 1080 joules of heat. from this data, calculate the specific heat of aluminum

4. What amount of heat is required to raise the temperature of 20 grams of water from 10°C to 30°C? The specific heat of water is 4.18 J/g°C.Select one of the options below as your answer: A. 1200 joules B. 1500 joules C. 2000 joules D. 2300 joules E. 3000 joules

1. Ethanol (C2H5OH) melts at -114 degrees Celsius. The enthalpy of fusion is 5.02 kj/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135 degrees Celsius to

2. At a pressure of 1ATM, _____ KJ of heat is needed to vaporize a 32.3 g sample of liquid ethanol at its normal boiling point of 78.4 C. Boiling point (78.4 C), specific heat (2.46 J/g C), and Hvap(78.4 C)=38.6 KJ/mol are provided. Please include how to

3. Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid

4. The latent heat of vaporization of ethanol is 200 calories/gram. This means that _____.

5. Submit pseudocode for the following programming exercise: Fat Gram Calculator Design a program that asks for the number of fat grams and calories in a food item. Validate the input as follows: - Make sure the number of fat grams and calories are not less

6. The latent heat of vaporization of H2O at body temperature (37°C) is 2.42 x 106 J/kg. To cool the body of a 77.6-kg jogger [average specific heat capacity = 3500 J/(kg C°)] by 2.78 C°, how many kilograms of water in the form of sweat have to be

7. At Wendy's a cheeseburger has 200 fewer calories than a large fries. Two cheeseburgers are a large fries have 1100 calories. How many calories are in each item? Let c represent the number of calories in a cheeseburger and let f represent the number of

8. The latent heat of fusion for water is 33.5 × 104 J/kg, while the latent heat of vaporization is 22.6 × 105 J/kg. What mass m of water at 0 °C must be frozen in order to release the amount of heat that 2.32 kg of steam at 100 °C releases when it

9. How much heat is required to convert 32.5 grams of ethanol at 28 C to the vapor phase at 78 C? Ethanol (C2H5OH) boils at 75 C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g-K.

10. Imagine that a hypothetical life form is discovered on our moon and transported to Earth. On a hot day, this life form begins to sweat, and it is determined that the heat of vaporization of its sweat is 155 cal/g. The scientist observing the

11. Compare the amount of heat required to vaporize a 200.-gram sample of H20(L) at its boiling point to the amount of heat required to melt a 200.-gram sample ofH20(s) at its melting point.

12. Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135 °C to liquid

1. Pretty general and with no context; however, this may fit.
   it requires 200 calories of energy to change the phase of 1 gram of ethanol at its boiling point from liquid to vapor.

2. The latent heat of vaporization of ethanol is 200 calories/gram. This means that about 200 calories of heat must be added to 1 gram of ethanol to convert it form a liquid to a gas.

3. But that is if the liquid is at the boiling point of ethanol. If the ethanol is t a temperature lower than the boiling point then more energy is required for every degree < the b.p.

1. Ethanol (C2H5OH) melts at -114 degrees Celsius. The enthalpy of fusion is 5.02 kj/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135 degrees Celsius to

2. At a pressure of 1ATM, _____ KJ of heat is needed to vaporize a 32.3 g sample of liquid ethanol at its normal boiling point of 78.4 C. Boiling point (78.4 C), specific heat (2.46 J/g C), and Hvap(78.4 C)=38.6 KJ/mol are provided. Please include how to

3. Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid

4. Submit pseudocode for the following programming exercise: Fat Gram Calculator Design a program that asks for the number of fat grams and calories in a food item. Validate the input as follows: - Make sure the number of fat grams and calories are not less

5. The latent heat of vaporization of H2O at body temperature (37°C) is 2.42 x 106 J/kg. To cool the body of a 77.6-kg jogger [average specific heat capacity = 3500 J/(kg C°)] by 2.78 C°, how many kilograms of water in the form of sweat have to be

6. At Wendy's a cheeseburger has 200 fewer calories than a large fries. Two cheeseburgers are a large fries have 1100 calories. How many calories are in each item? Let c represent the number of calories in a cheeseburger and let f represent the number of

7. The latent heat of fusion for water is 33.5 × 104 J/kg, while the latent heat of vaporization is 22.6 × 105 J/kg. What mass m of water at 0 °C must be frozen in order to release the amount of heat that 2.32 kg of steam at 100 °C releases when it

8. How much heat is required to convert 32.5 grams of ethanol at 28 C to the vapor phase at 78 C? Ethanol (C2H5OH) boils at 75 C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g-K.

9. Imagine that a hypothetical life form is discovered on our moon and transported to Earth. On a hot day, this life form begins to sweat, and it is determined that the heat of vaporization of its sweat is 155 cal/g. The scientist observing the

10. Compare the amount of heat required to vaporize a 200.-gram sample of H20(L) at its boiling point to the amount of heat required to melt a 200.-gram sample ofH20(s) at its melting point.

11. Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135 °C to liquid

12. steam at 100 degree C is passed into a container of negligible heat capacity containing 20 g of ice and 100 g of water at 0 degree C, until the ice is completely melted. Determine the total mass of water in the container. ( specific latent