Activity 1. Solve and answer the activity on a separate sheet and yourobservations on the diagrams presented.Solving Involving Heat and Change of State (Show Your Solution)1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at 20°C to convert it to liquid water at 60.0 °C.Given: Specific heat (ice) = 2.1 J/g•°C_Specific heat (water) = 4.18 J/g °CHus = 6.0 kJ/mol%3D

Answered: Image /qna-images/answer/f9ff1bda-9033-4a82-a728-44fb6f87a49d.jpg

1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at 20 °C to convert it to liquid water at 60.0 °C. Given: Specific heat (ice) = 2.1 J/g• °C_Specific heat (water) = 4.18 J/g• °C Hfus = 6.0 kJ/mol

1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at 20 °C to convert it to liquid water at 60.0 °C. Given: Specific heat (ice) = 2.1 J/g• °C_Specific heat (water) = 4.18 J/g• °C Hfus = 6.0 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

What amount of thermal energy (in kJ) is required to convert 221 g of ice at -16 °C completely to water vapour at 214 °C? The melting point of water is 0 °C and its normal boiling point is 100 °C. The heat of fusion of water is 6.02 kJ mol-¹ The heat of vaporization of water at its normal boiling point is 40.7 kJ mol-¹ The specific heat capacity of ice is 2.09 J g-¹ °C-¹ The specific heat capacity of liquid water is 4.18 J g-¹ °C-¹ The specific heat capacity of water vapour is 2.01 Jg¹¹ °C-¹ Answer:
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05 kg of water decreased from 117 °C to 56.5 °C. Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C
Two 20.0 g ice cubes at -20.0 °C are placed into 245 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 = x10 TOOLS °C
What amount of heat (in kJ) is required to convert 15.5 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)
How much energy would need to be added to 930.g of ice at 0.0°C to turn it into liquid water at 0.0°C ? 930. J O 3.89x103 J O 1.86x103 J O 2.10x106 J 3.12x105 J
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)?
1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at -20C to convert it to liquid water at 60.0C. Given: Specific heat (ice) = 2.1 J/g.C Specific heat (water) = 4.18 J/g-C Hfus = 6.0 kJ/mol or 334 J/g
Specific heat of H,O(s) 2.087 J/(g · °C) Specific heat of H,O(1) |4.184 J/ (g · °C) Heat of fusion for H,O A total of 865 cal of heat is added to 5.00 g of ice at -20.0 °C. 333.6 J/g What is the final temperature of the water? °C Tinal
What amount of heat (in kJ) is required to convert 10.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･ °C; specific heat capacity of liquid = 1.58 J/g･ °C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3 °C)
What amount of heat (in kJ) is required to convert 17.2 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°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.
How much heat must be supplied to 36 g of ice at -21°C to convert it to steam at 152°C? (Specific heats: ice = 2.0 J/g·°C; water = 4.2 J/g·°C; steam = 2.0 J/g·°C. Molar heat of fusion of water at 273 K = 6.01 kJ/mol. Molar heat of vaporization of water at 373 K = 40.7 kJ/mol.)