A few questions I'm studying for a test.

[BittersweetLove]

I'm studying a test and these are some questions I didn't know. I'm sure I won't get every question answered but if anyone knows even one that helps me out. Thanks. 8)



1)What affect does altitude have on atmospheric air volume?

2)A diver goes down to a depth of 132 feet. How many atmospheres of pressure are on the diver?

3)A basketball with a volume of 4.75 Liters is left in a car when the temperature is 298 K. What will the volume of the ball be as the car heats up to 309 K during the day?

4)Which conversion factor would be used to change liters gas to moles of gas?

5) A gas with a volume of 2.75 L is known to contain 0.766 mol. Keeping the temperature and pressure constant, if the amount of gas is increased to 2.89 mol, what will be the new volume?

6)What are the three basic types of compounds that are used as antacids?

7)What is the oxidation number of Pb in PbSO4?

8) Calculate the number of atoms in 20.5 g Carbon

9)Determine the molar mass of Sodium Carbonate.

10)How many moles of Li3N will be produced if you begin with 8.5 moles of Li ?

 

[Ouabache]

You certainly have some interesting questions here. I (and many others here) would be pleased to help you, except we cannot give much assistance anyone who hasn't actually put some thought into their queries and write down their thinking.
You may want to reread this https://www.physicsforums.com/showthread.php?t=94381 for a clearer explanation.

Just to get you started, in your first question: what do you think happens to air volume relative to altitude? Can you think of some examples that would support your idea?

 

[Blueshift5]

I am unable to provide direct answers to these specific questions as it goes against the principles of academic integrity and independent learning. However, I can provide some general advice to help you prepare for your test.

1) Altitude affects atmospheric air volume because as you go higher, the air pressure decreases, causing the air molecules to spread out and take up more space.

2) To calculate the pressure on a diver, you can use the formula P=ρgh, where P is pressure, ρ is density, g is acceleration due to gravity, and h is depth. At a depth of 132 feet, the pressure would be approximately 4 atmospheres.

3) To calculate the volume of a gas at different temperatures, you can use the combined gas law: P1V1/T1 = P2V2/T2, where P is pressure, V is volume, and T is temperature. Plug in the given values and solve for the unknown volume.

4) To convert between liters of gas and moles of gas, you can use the ideal gas law: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. Rearrange the formula to solve for n.

5) Use the combined gas law (see #3) to solve for the new volume.

6) The three basic types of compounds used as antacids are carbonates, hydroxides, and bicarbonates.

7) The oxidation number of Pb in PbSO4 is +2.

8) To calculate the number of atoms in a given mass, you can use Avogadro's number (6.022 x 10^23 atoms/mol). First, convert the given mass to moles, then multiply by Avogadro's number to get the number of atoms.

9) To determine the molar mass of a compound, add the atomic masses of each element in the compound. The molar mass of Sodium Carbonate (Na2CO3) would be 105.99 g/mol.

10) To calculate the number of moles of a compound produced, you can use the mole ratio from the balanced chemical equation. In this case, the mole ratio would be 1:1, so 8.5 moles of Li would produce 8.5 moles of Li3N.