Question

10 moles of a mixture of hydrogen and oxygen gases at a pressure of 1 atm at constant volume and temperature, reaction form 3.6 g of liquid water. The pressure of the resulting mixture will be closest to

Answer 1

"As per the question, you can use the equal of ideal gas law that shows the relationship between,

PV = nRT

Here Pressure, P = 1 atm, Volume, V = 3.6 gm, Temperature T = 273 K, n = 10 moles

Hence,

1 * 3.6 = 10 * R * 273

R = 3.6/2730

R = 0.003

"

Answer 2

Answer:

The resulting pressure is 0.97 atm.

Explanation:

We know-

2H2 + O2 ⇒ 2H2O

Let us assume nitially there are x moles of hydrogen

⇒(10-x) moles of O2 ⇔ 0 moles of water.

After the reaction has occured

(x-a)(10-x- a/2)a

Now

a=3.6/18 = 0.2

⇒ New moles = x-a+10-x-a/2 = 9.7

Now,

P1/P2 = x1/x2

After substitution of respective value of P1,  

⇒ P2=0.97