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1) 2) 3) An adiabatic process is one that involves no heat transfer. What is the

ID: 1075883 • Letter: 1

Question

1) 2) 3) An adiabatic process is one that involves no heat transfer. What is the relationship between work and internal energy in an adiabatic process? What is the change in internal energy (in J) of a system that releases 675 J of thermal energy to the surrounding and has 530J of work done on it? Why is it often more convenient to measure in H instead of E? Why can you use either °C or K for AT in calorimetry, but you cannot use them interchangeably in gas law problems? Write a balanced chemical equation and draw an approximate enthalpy diagram for 4) 5) a. The combustion of 1 mol ethane b. Freezing of 10ml of water 6) Write a balanced chemical equation and draw an approximate enthalpy diagram foir a. Sublimation of 22g dry ice (solid CO2 into CO2 gas) 7) 8) 9) b. Reaction of 1 mol of SO2 with O2- Define the difference between molar heat capacity, specific heat capacity and heat capacity. Calculate q(the heat) when 10 g of ice is cooled from 10°C to -75°C (cice -2.087 J/(g K)). A 295g aluminum engine part at 13.00oC absorbs 75.0kJ of heat. What is the final temperature of the aluminum part? (cal 0.900 J/(g K)) 10) A 27.7 g sample of radiator fluid (ethylene glycol) releases 688J of heat. What is the initial temperature if the final temperature is 32.5°C? (c for ethylene glycol is 2.42 J/(g K)) 11) when 155ml of water at 26.0°C is mixed with 75ml of water at 85°C, what is the final temperature? (for water d 1.00g/mL, c-4.184 J/(g K), assume no heat is released to the surroundings) 12) A 19.3 g sample of propylene glycol, which can be used as a radiator coolant, absorbed 1187 J of heat. What was the initial temperature of the propylene glycol if the final temperature was 116.5°C (ceg-2.51 J/g-c)? 13) A unknown volume of water at 18.2°C is mixed with 24.4ml of water at 35°C, If the final temperature 23.5°C what is the unknown volume? (for water d = 1.00g/mL , c=4.1841/(g K), assume no heat is released to the surroundings) 14) A 30.5g sample of an unknown alloy at 93.0°C is placed into 50g of 22.0°C water. The final temperature of the water and metal system is 31.1°C, what is the specific heat capacity of the metal?

Explanation / Answer

Answer 1.

According to the 1st law of Thermodynamics;

Q= U + W

In an adiabatic process: Q= 0

So,

U= -W

The first law of thermodynamics with Q=0 shows that all the change in internal energy is in the form of workdone.

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