The volume of gas is 200.0 ML and the pressure of 2.00 ATM. When the with volume of a gas is 10 ML what is the pressure of the temperature remains the same

40 atm.

Explanation:

From the question given above, the following data were obtained:

Initial volume (V₁) = 200 mL

Initial pressure (P₁) = 2 atm

Final volume (V₂) = 10 mL

Temperature = constant

Final pressure (P₂) =?

The final pressure of the gas can be obtained by using the Boyle's law equation as shown below:

P₁V₁ = P₂V₂

2 × 200 = P₂ × 10

400 = P₂ × 10

Divide both side by 10

P₂ = 400 / 10

P₂ = 40 atm

Thus, the final pressure of the gas is 40 atm.

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.

c. 75.7

i think that is the right