Determine the temperature (in K) of 0.6 moles of gas contained in a 1.7 L vessels at a pressure of 154.2 kPa.

51.6K

Explanation:

Given parameters:

number of moles = 0.6moles

Volume  = 1.7L

Pressure  = 154.2kPa

Unknown:

temperature = ?

Solution

The ideal gas law is best used to solve this kind of problem. The law combines Boyle's law, Charles's law and Avogadro's law.

         PV = nRT

wherre P = pressure in atm

           V = volume in dm³ or L

           n = number of moles

            R = gas constant

         T = temperature in kelvin

Since T is the unknown, we make it the subject of the expression;

             T =

            1atm = 101325Pa

             x atm  = 154.2 x 10³Pa

         x  =  = 1.52atm

T =   =   = 51.6K

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.

plants need sunlight, water, and carbon dioxide to make food. plants use the raw materials of water, nutrients they absorb from soil, and carbon dioxide to make sugars the plant can use. energy from the sun and chlorophyll are also needed.