A1.50 l sample of h₂ gas at 3.50 atm was combined with 2.00 l of n₂ gas at 2.55 atm pressure at a constant temperature of 25.0 °c into a 9.10 l flask. the total pressure in the flask is atm. assume the initial pressure in the flask was 0.00 atm. r = 0.08206 (l*atm)/(mol*k)

The total pressure in the flask is 1,14 atm

Explanation:

We need to apply the Ideal Gas law to get the moles and then find out the total moles in the mixture

moles H2 + moles N2

P.V = n. R . T

1,50 L . 3,50atm = n . 0,08206  (L*atm)/(mol*K) . 298K

(1,50 L . 3,50atm) / 0,08206 (mol*K)/(L*atm) . 298K = n

(5,25 / 24,45) mol = n = 0,215 moles H2

2,55 atm . 2,00 L = n . 0,08206  (L*atm)/(mol*K) . 298K

(2,55 atm . 2,00 L) / 0,08206 (mol*K)/(L*atm) . 298K = n

(5,1 / 24,45) mol = n = 0,208 moles N2

Total moles = moles H2 + moles N2

0,215 moles H2 + 0,208 moles N2 = 0,423 moles

P.V = n. R . T

P . 9,10L = 0,423moles . 0,08206  (L*atm)/(mol*K) . 298K

P = (0,423moles . 0,08206 (L*atm)/(mol*K) . 298K ) / 9,10L

P = 1,14 atm

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