A 519.93 gram sample of N2O is in a 7.05 L container. What is the pressure of the gas in atmospheres when the temperature is 125.63K?

The pressure of the gas is 17.27 atm

Explanation:

Step 1: Data given

Mass of N2O = 519.93 grams

Molar mass of N2O = 44.01 g/mol

Volume = 7.05 L

Temperature = 125.63 K

Step 2: Calculate moles N2O

Moles N2O = mass N2O / molar mass N2O

Moles N2O = 519.93 grams / 44.01 g/mol

Moles N2O = 11.81 moles

Step 3: Calculate pressure

p*V = n*R*T

p = (n*R*T)/V

⇒with p = the pressure of the gas = TO BE DETERMINED

⇒with n = the number of moles of gas = 11.81 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 125.63 K

⇒with V  = the volume = 7.05 L

p = (11.81 * 0.08206 * 125.63) / 7.05

p = 17.27 atm

The pressure of the gas is 17.27 atm

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acid : acids are those which accepts an electron-pairs.

base : bases are those which donates ab electron-pairs.

alkali : it is a base that dissolves in water. it is basically a base and the ph greater than 7.

hydroxide ion : it is a poly-atomic ion which is negatively charged.

the millers tale is the answer.