What pressure will be exerted by 0.60 mol of CO2 when its temperature is 25 OC and it is in a 500 mL container?

29.3 atm

Explanation:

We need to use the Ideal Gas Law to solve this problem: PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is the temperature in Kelvin.

Here, volume is V = 500 mL = 0.500 L; moles is n = 0.60 mol; R is 0.08206 atm/(mol * K); and temperature is T = 25 + 273 = 298 K. Plug these into the equation to solve for P:

P * (0.500 L) = (0.60 mol) * (0.08206 atm/mol * K) * (298 K)

P ≈ 29.3 atm

Hope this helps!

Explanation:

Relation of with is given by the formula:

where,

= equilibrium constant in terms of partial pressure

= equilibrium constant in terms of concentration

R = Gas constant

T = temperature

= change in number of moles of gas particles =

when = 0

a)

= change in number of moles of gas particles =

b)

= change in number of moles of gas particles =

c)

= change in number of moles of gas particles =

d)

= change in number of moles of gas particles =

Thus for reaction , , as = 0