Practice problem: A fixed volume of 5 L is holding 4 moles of gas at a pressure of 3 atm. If the quantity of gas is increased to 5 moles, what will be the new pressure?   Practice Problem (You first need to determine which law to use).  A 0.4 moles of gas with a volume of 2 L has a T of 413 K and a P of 7 atm. If we decrease the T to 325 K while holding the V constant, what is the new P?

8 Problem 8: The pressure of a gas is reduced from 6.7 atm to 4.45 atm as the volume of its container is increased by moving a piston from 8.5 L to 12 L. What would the original temperature be if the final temperature is 385 K.

3:18 AM Tue Jan 31 Question 3 of 17 What is the temperature (in K) of 0.380 mole of neon in a 2.00 L vessel at 4.68 atm? O

Item 2 2 of 16 Learning Goal: I Review I Constants I Periodic Table To use partial pressure in gas law calculations. partial pressure of Ar is 0.400 atm . What is the partial pressure of Xe? In a mixture of gases, the total pressure of the gas mixture is equal to the sum of the partial pressures of the individual Express your answer to three significant figures and include the appropriate units. gases. For example, if you have a mixture of • View Available Hint(s) helium at 2 atm and argon at 4 atm , then the total pressure of the gas inside the cylinder is 6 atm . (Figure 1) Similarly, if you know the total pressure of a gas mixture, you can use the number of moles to find the partial pressures, or the partial pressures to find the number of moles. HẢ ? Pxe Value Units Example Problem: A mixture of N2, O2, and He gases has a total pressure of 1 atm . The partial pressures of N, and O, are 0.7 atm and 0.25 atm, respectively. Figure 1 of 1 Part B 7. A volume of 18.0 L contains a mixture…

What is the volume of a 4.000 L balloon of oxygen when the pressure is increased from 2.000 atm to 6.000 atm at a constant temperature of 25.00 oC ? This is a change in conditions problem, we need to define the variables: V1 =  _____________ L           T1 = _____________ K            P1 =  ____________ atm V2 = ? L                                                 T2 =  _______________ K            P2 =  ______________ atm The problem doesn't mention the moles, n, thus the amount of moles was not changed and n1 =  _____________. Constant volume means V1 = V2 The equation simplifies to   P2 V2       P1 V1              P2 V2    P1 V1                                       __________   _______________ –––––– = ––––––        –––––– = ––––––         solving for V2 = –––––––––––––––––––––––––––––––––––––––––––––––  n2 T2       n1 T1                1             1                                                 _________________                                                   ______________…

Practice Problems 1. A gas has a volume of 350 ml at 30 C. If the volume changes to 400 ml, what is the new temperature? 2. Submarines need to be extremely strong to withstand the extremely high pressure of water pushing down on them.  An experimental research submarine with a volume of 1,510 liters has an internal pressure of 1.20atm.  If the pressure of the ocean breaks the submarine forming a bubble with a pressure of 253atm pushing on it, how big will that bubble be? 3. A sample of nitrogen inside a rigid, metal container at 20.0ºC is placed inside an oven whose temperature is 50.0 ̊ C. The pressure inside the container at 20.0ºC started at 3.00 atm?

3 Problem 3: A gas that has a volume of 34 L, a temperature of 318 K and an unknown pressure, has its volume increased to 40 L and its temperature decreased to 308 K. The pressure after the change is 2 atm. What is the original pressure of the gas?

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