Question

Question #8097e

Answer 1

I think the question is for ideal gas equation and details are given below

Explanation:

Boyle's law states that pressure of ideal gas is inversely proportional to volume at constant temperature and concentration of gas

`V prop 1/P` (Constant Temp and n i.e no of mole of gas)

Charles law states that volume of the an ideal has is directly proportional to temperature at constant pressure

`V prop T` (constant pressure, n) here temperature should be in kelvin scale

Avogadro law states that the equal volume of gas at same temperature and pressure contains equal number of mole of gas

`V prop n` ( Constant T and P)

when these equations we get ideal gas equation

PV = nRT where R is called as the gas constant by using this

This gas law applicable for at very high temperature and low pressure because of assumption of inter molecular attraction is lower and volume occupied by the gas molecules is negligible. But obey ideal gas equation are known as ideal gases, whereas the gases which do not obey this law is known as real gases.

Answer 2

The formula for the combined gas law is `(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`.

Explanation:

The combined gas law comes from Charles', Boyle's, and Gay Lussac's laws.

The formula is `(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`. (Temperature is in Kelvins.)

If you have a problem involving the combined gas law, determine which variables you know, and which one you don't know. Then rearrange the equation to isolate the unknown variable, then solve for the unknown variable.

Practice Problem
What is the volume of gas at 2.00 atm and 200.0 K if its original volume was 300.0 L at 0.250 atm and 400.0 K.

Solution:

Identify what is known.

`"initial volume:"` `V_1="300.0 L"`
`"initial pressure:"` `P_1="0.2500 atm"`
`"initial temperature:"` `T_1="400.0 K"`
`"final pressure:"` `P_2="2.000 atm"`
`"final temperature:"` `T_2="200.0 K"`

Identify what is unknown.
`"final volume:"` `V_2"`

Equation:

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`

Solution:
Rearrange the equation to isolate `V_2`, then solve for `V_2`.

`V_2=(P_1V_1T_2)/(T_1P_2)=(0.2500cancel"atm"*300.0"L"*200.0cancel"K")/(400.0cancel"K"*2.000cancel"atm")="18.75 L"` to four significant figure.