1)What is a gas? How do we know there is gas pressure on us? How could you demon

Question

1)What is a gas? How do we know there is gas pressure on us? How could you demonstrate this?

2) Would it be easier to drink water with a straw on top or at the foot of Mt. Everest? Explain. What is the atmospheric pressure on Mt Everest anyway? Give this value in atmospheres and mmHg.

3) A gas occupying a volume of 725 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?

4) A 36.4 L volume of methane gas is heated from 25oC to 88oC at constant pressure. What is the final volume?

5) If a balloon started out with a volume of 1.3 liters at room temperature. What would be the volume of the air inside if the temperature of the liquid nitrogen is -196oC. Is the “air” even a gas anymore? If not, what is it?

6) A whale is able to dive to depths of 1000 meters, where the pressure is 100 atm and the temperature is 20oF. If the whale takes a breath and fills its lungs with a volume of 400 L at the surface, where the temperature is 65oF, and the pressure is 1 atm, What is the volume of its lungs at this depth?

7) I decide to blow up a balloon. The volume initially was 21.2-L and it changes to 39.5 L. The balloon initially weighed 1.35 g and was filled with oxygen gas. I added hydrogen gas to reach the new volume. How many grams of hydrogen gas must have I added? Assume constant temperature and a pressure of 758 mmHg.

8) Calculate the constant temperature in 7) ? Does this make sense given the amount of gas and the volume of the balloons?

9) Calculate the volume(in liters) occupied by 2.12 moles of nitrogen monoxide at 6.54 atm and 76oC.

10) What is the volume(in liters) occupied by 49.8 g of HCl at STP? See Problem 5.40

11) If 6.9 moles of carbon monoxide gas is present in a volume of 30.4 L. What is the pressure of the gas at a temperature of 62oC? See Problem 5.32

12) A certain amount of gas at 25oC and at a pressure of 0.800 atm is contained in a glass vessel that can withstand pressures of 2.00 atm. How high can you raise the temperature without bursting the vessel?

13) a) Balance the following equation by inserting the correct coefficients, even if it is the number one.

___ NaHCO3(s) + ____ HC2H3O2(l) ------->____ CO2(g) + ___ NaC2H3O2(s) + ____H2O(l)

b) I used 1 gram of each reactant. Calculate the volume of CO2 gas that resulted from each reactant at

room temp - which was 65oF and oven temp - which was 325oF. You are at seal level. You will have two calculations. Decide which reactant is the limiting. ________________

number of moles of B. Soda:           number of moles of vinegar:

Volume of gas produced from B. Soda at both temps(PV=nRT)

65oF                                           325oF

Volume of gas produced from vinegar at both temps(PV=nRT)

65oF                                           325oF

Choose which volume above is the volume of my cake after baking(assume the cake "caught" all the gas, like a balloon)?

How could I increase the volume of gas produced to make my cake rise more?

What would the volume of the cake be in los angeles?

14) Given the following:

   2NO(g) + O2 (g) -> 2NO2 (g)

If 9 L of NO are reacted with an excess of oxygen at STP, what is the volume in liters of the NO2 produced? See Problem 5.53

15) Nitroglycerine, an explosive compound, decomposes according to the equation:

   4C3H5(NO3)3(s) -> 12CO2(g) + 10H2O(g) + 6N2(g) + O2(g)

Calculate the total volume of all gases combined when collected at 1.2 atm and 25oC from 260g of nitroglycerine.

What are the partial pressures of the gases under these conditions?

Can the individual volumes of each gas be calculated?

Finally, based on the above equation, explain why you think nitroglycerine is such a powerful explosive?

16) Why does H2 move faster than Cl2? What effect does temperature have on this?

17) Describe gas diffusion. Is this faster in the winter or summer? Explain.

18) Describe on the molecular level what happens to a gas when it is put under high pressure or low temperatures? Why does this cause a deviation from ideal behavior? Draw a picture to help me understand.

19) At 27oC, 10.0 moles of a gas in a 1.50 L container exert a pressure of 130 atm. Is this exhibiting ideal gas behavior? Do a calculation to back up your answer and explain.(# moles or pressure?)

20) Use the van der waals equation to calculate the pressure exerted by 2.50 moles of CO2 confined in a volume of 5.00 L at 450 K. Also do the calculation with the ideal gas equation and compare and discuss the differences. Is this gas exhibiting ideal behavior? Explain.

Explanation / Answer

Hi! Can you please post them as separate chegg questions? that way more experts will be able to help you. Thanks!!

1) Is a state of matter in which the particles have a weakly interaction between them, that way each particle is separated from each other ocuppying the entire volume of the room where is contained.

2) Pressure in mount everest is 252.77 torr; 0.33 atm

No, it will not be easier because the pressure over the liquid is smaller than a 0 m over the sea so it is difficult to make a difference of pressure between the mouth and the atmospheric pressure.

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