What would be the temperature of 0.734 moles of chlorine gas be at 1.83 atmospheres in a 10.2 liter container? (r=0.0821 L·atm/mol·k)

310K

Explanation:

Since,

Pressure P = 1.83 atmospheres

Volume of chlorine gas V = 10.2L

Molar gas constant R = 0.0821 L.atm/mol.k)

Number of moles = 0.734 moles

Temperature T(in Kelvin) = ?

Apply ideal gas equation (pV = nRT)

1.83atm x 10.2L= 0.734 moles x 0.0821 L.atm/mol.k x T

18.67 = (0.06026 x T)

T = (18.67 / 0.06026)

T = 310K

Therefore, the new temperature of the chlorine gas is 310K

*tilts head* sounds more like a statement

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation: