A closed container in lab contains a sample of oxygen gas. When the temperature in lab is 16.3 degrees Celcius, the pressure in the container is 9.30 atm. What would the temperature in lab be (in Celcius) if the pressure in the container was 17.7 atm? Assume the mol and volume of the container are constant. Record your answer as a number with the correct significant figures.

T₂  = 550.60 K

Explanation:

Given data:

Initial temperature = 16.3°C (16.3+273 = 289.3 K)

Initial pressure = 9.30 atm

Final temperature = ?

Final pressure = 17.7 atm

Solution:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

9.30 atm / 289.3 K = 17.7 atm/T₂

T₂ =  17.7 atm × 289.3  K / 9.30 atm

T₂  = 5120.61 atm. K /9.30 atm

T₂  = 550.60 K

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.

the ozone layer acts as a filter for the shorter wavelength and highly hazardous ultraviolet radiation (uvr) from the sun, protecting life on earth from its potentially harmful effects. when the sky is clear, there is an inverse relationship between stratospheric ozone and solar uvr measured at the earth's surface.