What is the: Heat lost by Water (j) Change in Ice Temp (Celsius) Heat Gained by...

What is the:

Heat lost by Water (j)

Change in Ice Temp (Celsius)

Heat Gained by Ice after Melted (j)

Heat Used to Melt Ice (j)

Theoretical heat to Melt Ice (j)

% error

given the Initial volume of water = 70mL final volume of water = 100mL

given the initial temp of water = 24 degrees C final temp of water = 6 degrees C

Solutions

Expert Solution

Here essentially the theoretical yield is same as the calculated value. This is because I calculated the mass of ice, which is a theoretical value. Usually in an experiment such values will be give and we can calculate part 3 and 4 easily.

3) Heat gained by ice after melting = mass of ice * 4.2 * 6

ie. m * c * ∆T

4) Heat used to melt ice = mass of ice * 336

Put the value of mass here and you will get the answer.

PS : If you have any doubt just comment below.

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

1. Calculate the heat lost by the hot water. 2. Calculate the heat gained by the...

1. Calculate the heat lost by the hot water. 2. Calculate the heat gained by the cold water. 3. Calculate the heat gained by the calorimeter. 4. Calculate the calorimeter constant. Data: Atmospheric Pressure- 100.87 kPa Boiling point of water at this pressure- 99.8°C Mass of empty calorimeter- 8.3676 grams Mass of calorimeter plus 40 mL of water- 48.6923 grams Mass of calorimeter after adding 50 mL of hot water- 98.0557 grams Temperature of cold water just before adding addition...

1. Specific heat of water is 4.184 J/g ˚C. What is the heat in KJ gained...

1. Specific heat of water is 4.184 J/g ˚C. What is the heat in KJ gained when 20 q of water is heated from 22˚C to 77˚C? 2. What is the heat in J to melt 100g of NaCl when the HF for NaCl is 518 J/g? 3. What is the heat in J to equate 50 g Acetic Acid when the HE = 390 J/g?

Take the heat capacity of ice as 2.108 J/(g*C) and the heat capacity of water as...

Take the heat capacity of ice as 2.108 J/(g*C) and the heat capacity of water as 4.184 J/(g*C) for this problem. For water, DHfus = 6.001 kJ/mol at 0 C. a. A 10.0 gram ice cube at -10.0 C is placed into 45.0 mL of water at 40 C. Determine the final physical state and temperature of the result. Calculate DS for the ice cube and the surrounding water, and Use the value DStot to explain why this process is...

Heat of Fusion of Ice A. Determine the number of calories and joules lost by the...

Heat of Fusion of Ice A. Determine the number of calories and joules lost by the warm water. B. Determine the number of calories and joules needed to warm the melted ice. C. Determine the number of calories and joules required to melt the ice. D. Calculate the heat of fusion of ice in cal/g and J/g. Heat of Fusion of Ice Initial volume of water (Trial 1 &2) = 25 ml, 25 ml Initial water temperature (Trial 1 &...

how much heat is necessary to change 450g of ice at -11 degrees c to water...

how much heat is necessary to change 450g of ice at -11 degrees c to water at 20 degrees Celsius?

what is the eventually change during the process in which 100g of water at 50.0degree Celsius...

what is the eventually change during the process in which 100g of water at 50.0degree Celsius is cooled to ice at -30 degree Celsius

In an experiment, 300 g of aluminum (specific heat of 900 J/kg*K) at 120 Celsius is...

In an experiment, 300 g of aluminum (specific heat of 900 J/kg*K) at 120 Celsius is mixed with 60 g of water at 20 Celsius, with the mixture thermally isolated. You will need to look up the specific heat of water. (a) What is the equilibrium temperature? (b) What is the entropy change for the aluminum block? (c) What is the entropy change for the water? (d) What is the entropy change for the aluminum-water system?

Explain heat transfer, latent heat and change in temperature for the following case: Ice kept at...

Explain heat transfer, latent heat and change in temperature for the following case: Ice kept at -10 degrees C temperature turns into water at +10 degrees C temperature upon heating.

What heat energy must be added to 64 g of ice at 0°C to change it...

What heat energy must be added to 64 g of ice at 0°C to change it to water vapor (steam) at 100°C?

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 20.4 g of steam at 162°C is condensed, cooled, and frozen to ice at -50.°C.

Subjects