What is the volume of 0.366 moles of helium collected at 25 C and a
pressure of 0.98 atm?*

V = 9.14 L

Explanation:

Given data:

Volume of helium = ?

Number of moles = 0.366 mol

Temperature = 25°C (25+273 = 298 K)

Pressure of gas = 0.98 atm

Solution:

Formula:

PV = nRT

R = general gas constant = 0.0821 atm.L/ mol.K

V = nRT/P

V = 0.366 mol ×  0.0821 atm.L/ mol.K  × 298 K / 0.98 atm

V = 8.95 L / 0.98

V = 9.14 L

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.

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.