Watch how the solubility of a gas changes as pressure is increased and then decreased during the run.

which of the following statements correctly explain the relationship between the solubility of a gas and its pressure?

check all that apply.

check all that apply.

as pressure is increased, the rate at which gas molecules enter the solution decreases.
as pressure decreases, the concentration of gas molecules in the solution increases.
the solubility of a gas decreases with a decrease in pressure.
more gas molecules are soluble as pressure is increased.
the solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm.
the concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm.
fewer gas molecules are soluble at higher pressures.

-More gas molecules are soluble as pressure is increased.

-The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm.

-The solubility of a gas decreases with a decrease in pressure.

-The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm.

Explanation:

Henry's law

The solubility of a gas in a liquid solvent at a given temperature is directly proportional to the partial pressure of the gas over the solution. This relationship is expressed by a simple equation known as Henry's law:

S=k×P

yes they ca   is ur ansswerrr

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :