Initially, a 55.0 liter compressible container, holding 2.4 moles of a gas, exerts a pressure of 760 millimeters of mercury at a temperature of 280 kelvin. what is the pressure when the container is compressed to 43.0 liters, the moles of gas reduces to 1.8 moles, and the temperature changes to 36 degrees celsius?
93.7 mm hg
492 mm hg
740 mm hg
805 mm hg

805 mmHg is the pressure when the container is compressed

Explanation:

Initial Volume of the gas, V = 55.0 L

Initial Moles of the gas, n = 2.4 mol

Initial Pressure of the gas ,P=760 mmHg

initial temperature of the gas, T = 280 K

Using an Ideal gas equation:

...(1)

Final Volume of the gas, V '= 43.0 L

Final Moles of the gas, n' = 1.8 mol

Final Pressure of the gas = p'

Final temperature of the gas, T' =36 °C = 309 K

Using an Ideal gas equation:

..(2)

(1)=(2)

P' = 805 mmHg

805 mmHg is the pressure when the container is compressed.

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.