9) a 22.8 ml volume of argon gas is collected at 48.0o c. at constant pressure, what volume would this same sample of gas occupy at standard temperature?

19.39 mL.

Explanation:

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R  is the general gas constant,

T is the temperature of the gas in K.

(V₁T₂) = (V₂T₁)

V₁ = 22.8 mL, T₁ = 48°C + 273 = 321 K,

V₂ = ??? mL, T₂ = 273 (standard temperature = 273 K),

(V₁T₂) = (V₂T₁)

∴ V₂ = (V₁T₂)/(T₁) = (22.8 mL)(273 K)/(321 K) = 19.39 mL.

answer: you could do some invislibe ink.

explanation: i will tell you how to if u answer my question.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.