A sample of 1.00 moles of oxygen at 50°C and 98.6 kPA occupies what volume?

27.3L

Explanation:

Looking at the parameters given;

Number of moles (n)= 1.00 moles

Temperature (T) =50° +273= 323K

Pressure (P)= 98.6KPa or 0.97 atm ( to obtain this, divide 98.6×10^3/101325)

R= 0.082 L.atmK-1mol-1

Then we apply the ideal gas equation

PV=nRT

V= nRT/P

V= 1.00×0.082×323/0.97

V= 27.3L

The volume occupied by the gas is 27.25 L.

Explanation:

The ideal gas equation dictates that the kinetic energy is directly proportional to the temperature in an ideal gas.

And an ideal gas is a hypothetical gas made up of point particles with no attraction or repulsion between them.

The ideal gas equation is: PV = nRT

To find the volume occupied by a gas, the values of the variables Temperature (T), Pressure (P), a constant (R: The universal constant of ideal gases), and the number of moles (n) must be taken.

The data they give us is:

Then the variable we want to find is cleared, that is, the volume:

Then the data is placed:

And the answer is given in units of volume:

jdjxnbfb

explanation:

jjfnc fdnxnxx

indium, and thallium have three electrons i think