1. An ideal gaseous reaction (which is a hypothetical gaseous reaction that conf

Question

1. An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 45.0 atm and releases 63.9 kJ of heat. Before the reaction, the volume of the system was 9.00 L . After the reaction, the volume of the system was 2.00 L .

Calculate the total internal energy change, U, in kilojoules.

PUT UNITS AFTER ANSWER

2. An ideal gas (which is is a hypothetical gas that conforms to the laws governing gas behavior) confined to a container with a massless piston at the top. (Figure 2)  A massless wire is attached to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 4.90 to 2.45 L . When the external pressure is increased to 2.50 atm, the gas further compresses from 2.45 to 1.96 L .

In a separate experiment with the same initial conditions, a pressure of 2.50 atm was applied to the ideal gas, decreasing its volume from 4.90 to 1.96 L in one step.

If the final temperature was the same for both processes, what is the difference between q for the two-step process and q for the one-step process in joules?

3. Calculate the work in kilojoules done during a synthesis of ammonia in which the volume contracts from 8.4 L to 4.3 L at a constant external pressure of 46 atm .

Express your answer using two significant figures.

Express your answer with the appropriate units.

Explanation / Answer

I am supposed to answer only 1 question at a time. So I will answer question 1 for you. please ask other questions separately again.

Question 1:
Q= -63.9 KJ = -63900 J
Heat released is taken as negative

Work done, W = - P(Vf- Vi)
                      = - 45 (2-9)
                      = 315 atmL

Since 1 atmL equals 101.3 J

W becomes 315*101.3 = 31909.5 J

delta U = Q+ W
    = -63900 J + 31909.5 J
    = -31990.5 J
    = -32 KJ

Answer: -32 KJ

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