The stratosphere, between 6 and 10 miles from the surface of earth
If you decreased the volume of a sample of gas by a factor of three while maintaining a constant pressure, how would the absolute temperature of the gas be affected?
✔ it would decrease threefold
A gas at 300 K and 4.0 atm is moved to a new location with a temperature of 250 K. The volume changes from 5.5 L to 2.0 L. What is the pressure of the gas at the new location?
✔ 9.2 atm
What is the partial pressure of 0.50 mol Ne gas combined with 1.20 mol Kr gas at a final pressure of 730 torr?
✔ 215 torr
Assuming the M is molarity, molarity is equal to mols/volume in liters.
So it would be 50M NaCl = X mols/ 1.0L
50M * 1.0L = X mols
X = 50
50 Mols of NaCl
Now that you have mols, you can then convert mols to grams by doing 50mols NaCl * (58.44 g NaCl/ 1 mol NaCl)
= 2922 grams of NaCl
Answer : The volume of water produced by this reaction would be, 4.75 liters.
Explanation : Given,
Volume of HCl gas = 9.5 L
The balanced chemical reaction will be:

As we know that at STP, 1 mole of gas occupy 22.4 L volume of gas.
By the stoichiometry we can say that:
As, 4 liter volume of HCl gas react to give 2 liter volume of water
So, 9.5 liter volume of HCl gas react to give
volume of water
Therefore, the volume of water produced by this reaction would be, 4.75 liters.
Answer:
2.6 atm
Explanation:
At constant temperature, solubility of gas increases as pressure increases, Hence, they varies directly proportional.
i.e S ∝ P


where:
S₁ and P₁ are the initial solubility and pressure of the gas
S₂ and P₂ are the final solubility and pressure of the gas
Making P₂ the subject of the formula from the above equation; we have:

where; it is given from the question that:
P₁ = 1.0 atm
S₁ = 0.36 g/L
S₂ = 9.5 g/L
Replacing the values into the above equation; we have:

P₂ = 2.6 atm
∴ The pressure needed to produce an aqueous solution containing 9.5 g/L of the same gas at 0°C = 2.6 atm