What is the total pressure in a 8.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C?

0.998 atm.

Explanation:

Using ideal gas law,

PV = nRT

Where,

P = pressure

V = volume

n = number of moles

R = gas constant

T = absolute Temperature in K.

Given:

T = 20°C

Temp, K = C + 273.15

= 293.15.

V = 0.0 L

The total number of moles of gas, n = number of moles of H2 + N2

= 0.127 + 0.288

= 0.415 moles.

R = the universal gas constant = 08206 L.atm/mol.K.

Therefore, using the equation above;

(P * 10.0) = 0.415 * 0.08206 * 293.15

= 0.998 atm.

the answer is a! (2.9 x 10^-18 j) hope i could someone. : )