Given the balanced equation: 3H2(g) + N2(g) → 2NH3(g)

Calculate the mass of NH3 produced by the complete reaction of 2. 55 g of H2.

14.45g

Explanation:

We have a balanced equation:

3H2(g) + N2(g) → 2NH3(g)

We know the mass H2 = 2.55g

We can work out the moles of H2 - Mass = mr  x moles

Moles = mass/ mr = 2.55/ 2 = 51/40

Using the ratios in the question, this is 3:2

51/40 /2 x 3 = 17/20

so there are 17/20 moles NH3

Mass = mr x moles = 17/20 x 17 = 289/20 = 14.45g

Hope this helps! Let me know if you have any questions :)

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

the answer is symmetrical : )