Ch4 with pressure 1 atm and volume 10 liter at 27°c is passed into a reactor with 20% excess oxygen, how many moles of oxygen is left in the products?

Answer : The moles of left in the products are 0.16 moles.

Explanation :

First we have to calculate the moles of .

Using ideal gas equation:

where,

P = pressure of gas = 1 atm

V = volume of gas = 10 L

T = temperature of gas =

n = number of moles of gas = ?

R = gas constant = 0.0821 L.atm/mol.K

Now put all the given values in the ideal gas equation, we get:

Now we have to calculate the moles of .

The balanced chemical reaction will be:

From the balanced reaction we conclude that,

As, 1 mole of react with 2 moles of

So, 0.406 mole of react with moles of

Now we have to calculate the excess moles of .

is 20 % excess. That means,

Excess moles of = × Required moles of

Excess moles of = 1.2 × Required moles of

Excess moles of = 1.2 × 0.812 = 0.97 mole

Now we have to calculate the moles of left in the products.

Moles of left in the products = Excess moles of - Required moles of

Moles of left in the products = 0.97 - 0.812 = 0.16 mole

Therefore, the moles of left in the products are 0.16 moles.

idk

explanation:

a polar bond is formed when electrons are shared unevenly between atoms