If five moles of a gas at a pressure of 5.4 kpa have a volume of 120 liters, what is the temperature?

Explanation:

Given parameters:

number of moles of gas = 5 moles

pressure on the gas = 5.4kpa

volume of gas = 120L

Unknown:

temperature of the gas = ?

Solution:

To solve this problem, we have to apply the ideal gas law.

The law is derived from the combination of the three gas laws: Boyle's law, Charles's law and Avogadro's law.

 Combining the laws, we have;

                  PV = nRT

where P is the pressure in atm

           V is the volume

           n is the number of moles

           R is the gas constant 0.082atm dm³ mol⁻¹ K⁻¹

          T is the temperatue in kelvin

Now, we must convert the pressure from kpa to atm;

          1 atm = 101.325kpa

                5.4kpa;

                              = 0.053atm

    Input the parameters;

            0.053 x 120 = 5 x 0.082 x T

                   T = 15.5K

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

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