Which of the following is/are statements of the 1st Law of Thermodynamics?

•  $\Delta E\ =\ q\ +\ w$  

• Heat and work are forms of energy

• Energy cannot be created nor destroyed, it can only be transformed.

• Total energy is always zero.

If q = 1100 J and w = 300 J for a given system, what is the change in internal energy for the system?

• +1400 J

• + 800 J

• - 800 J

• - 1400 J

What does $\Delta E$  stand for in the equation,  $\Delta E\ =\ q\ +\ w$ ?

• Change in Entropy

• Change in Element

• Change in Internal Energy

• Change in Free Energy

A gas absorbs 500 J of heat and does 200 J of work. What is the change in internal energy of the gas?

• + 700 J

• -700 J

• - 300 J

• + 300 J

The internal energy of a system decreases by 40 J. What work is done by the gas if the system absorbs 150 J of heat?

• - 110 J

• + 110 J

• - 90 J

• - 190 J

The internal energy of a gas increases by 50 J while the gas does 350 J of work. What can you say about the heat involved in the system?

• The gas releases 300 J of heat.

• The gas absorbs 300J of heat.

• The gas absorbs 400 J of heat.

• The system releases 400 J of heat.

If 600 J of heat is needed to increase the internal energy of a system from 15 J to 45 J. What amount of work will the system need to do on its surroundings?

• 630 J

• 570 J

• 660 J

• 540 J

The total amount of energy of a gas increases by 125 J as the gas does 40 J of work on its surroundings. Is the process exothermic?

• Yes

• No

• Not enough information given.

Given that 1 calorie = 4.184 J

How many calories is 1234 J?

• 294.9 J

• 5163 J

• 0.003391 J

• 1238 J

Given that 1 calorie = 4.184 J

How many J is 1234 calories?

• 0.003391 J

• 1238 J

• 294.9 J

• 5163 J