The pressure of a sample of argon gas was increased from 3.84 atm to 8.68 atm at

Question

The pressure of a sample of argon gas was increased from 3.84 atm to 8.68 atm at constant temperature. If the final volume of the argon sample was 10.1 L, what was the initial volume of the argon sample? Assume ideal behavior.

2. A hot air balloon is filled with 1.47 × 106 L of an ideal gas on a cool morning (11 °C). The air is heated to 119 °C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

3. If 31.5 moles of an ideal gas occupies 51.5 liters at 493 K, what is the pressure of the gas?

4. Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia.

N2(g)+3H2(g)--->2NH3(g) Assume 0.120 mol of N2 and 0.377 mol of H2 are present initially.

After complete reaction, how many moles of ammonia are produced?

How many moles of H2 remain?

How many moles of N2 remain?

What is the limiting reactant?

5.Calculate the mass, in grams, of 1.75 mol of xenon, Xe.

Explanation / Answer

1. P1V1= P2V2 (applying Boyle's Law)

P1= 3.84 atm , V1= ?

P2= 8.68 atm, V2= 10.1L

V1= 8.68*10.1/3.84= 22.83 L

2. V1/T1= V2/T2 (applying Charle's Law)

1.31 x 10^6 / 284 = V2 / 392

V2= 1.31 x 10^6*392/284= 1.80*10^6 L

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.