A 48.5-g sample of ice at -10.0°C is mixed with 110.0 g water at 85.0°C. Calculate the final temperature (in °C) of the mixture assuming no heat loss to the surroundings. The heat capacities for H₂O(l) and H₂O(s) are 4.184 J/g °C and 2.03 J/g °C, respectively, and the enthalpy of fusion of ice is 6.02 kJ/mol.

A 48.5-g sample of ice at -10.0°C is mixed with 110.0 g water at 85.0°C. Calculate the final temperature (in °C) of the mixture assuming no heat loss to the surroundings. The heat capacities for H₂O(l) and H₂O(s) are 4.184 J/g °C and 2.03 J/g °C, respectively, and the enthalpy of fusion of ice is 6.02 kJ/mol.

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...

See similar textbooks

Similar questions

A 11.3-g sample of ice at -12.0°C is mixed with 113.5 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 H₂O(s) and H₂O(l) are 2.03 and 4.18 J/g.°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol. Final temperature = °C
What 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)
A 5.00 g sample of water vapor, initially at 155*C is cooled at atmospheric pressure, producing ice at -55*C. Calculate the amount of heat energy lost by the water vapor sample in this process, in kJ. Use the following data specific heat capacity of ice is 2.09 J/ gK; the specific heat capacity of liquid water is 4.18 J/ gK; the specific heat capacity of water vapor is 1.84 J/ gK; the heat of fusion of ice is 336 J/g; the heat of vaporization of water is 2260 J/g. ( I know the answer is 15.6 kJ but I don't know how to get to it, Pls help ASAP!!)show all the steps you can pls
#98
Under normal atmospheric pressure, nitrogen boils (and condenses) at - 196°C. When 7.7 g of nitrogen gas at -196°C was put into a dewar flask nitially at -260°C, their temperatures reach -210°C. If the specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-°C and 200 J/g, espectively, determine the heat capacity of the dewar flask.
Two 20.0 g ice cubes at -14.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol.K) 75.3 J/(mol.K) 6.01 kJ/mol Tf= °C
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
Two 20.0 g ice cubes at -18.0 °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, Tf, of the water after all the ice melts. heat capacity of H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Tf = °C
With around 70% of ammonia produced industrially being used to make fertilizers. The specific heat capacity of liquid ammonia is 80.8 J/g*K while that of gaseous ammonia is 37.0 J/g*K. Given that the boiling point and enthalpy of vaporization of ammonia is -33.3°C and 23.5 kJ/mol, respectively, how much energy is required to heat 75 g of ammonia (17.03 g/mol) from the temperature of liquid nitrogen (-195.8°C) to room temperature (25.0°C)?
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.
8.) AHvap is a way to measure intermolecular forces quantitatively. Calculate the amount of energy (in kilojoules) needed to cool 550 g of water vapor from 150°C to -20°C. Assume that the specific heat of water is 4.184 J/g °C over the entire liquid range and the specific heat of steam is 1.99 J/g °C. The AHvap for water is 40.79 kJ/mol. The AHfus 6.01 kJ/mol. The specific heat of ice is 2.01 J/g °C
How much heat (in kJ) is released in converting 1.00 mol of water as a gas at 105°C to ice at –5.0°C? The heat capacity of H2O (g) is 2.01 J/g · °C The heat capacity of H2O (l) is 4.18 J/g · °C The heat capacity of H2O (s) is 2.09 J/g · °C The heat of fusion for water at 0 °C is approximately 0.334 kJ/g The heat of vaporization for water at 100 °C is 2.230 kJ/g.