Nitrogen (N2) and hydrogen (H2) combine at high temperatures, in the presence of

Question

Nitrogen (N2) and hydrogen (H2) combine at high temperatures, in the presence of a catalyst, to produce ammonia (NH3). All products and reactants are gases. Keq of above equation (at 500°C) is 1.45x10-5 Ka of NH4+ is 5.6x10-10

A. Write a balanced chemical reaction for this reaction.

B. Given 33.6 g of N2 and 6.0 grams of H2 in a 500mL container,

C. What is the limiting reagent?

D. Assuming 100% efficiency, how much ammonia would be produced?

E. How many grams of each reactant would be left over?

F. In your experiment you realize you don’t have as much product as 100% efficiency would have predicted. Explain why not and make a better prediction of how much NH3 will be produced (show your work). USE AN ICE TABLE

G. What is the percent yield you are predicting?

H. If you put all the product in 100 mL water, write a chemical equation showing what will happen AND determine the pH of this new solution?

I. What is the molar concentration of this new solution?

Explanation / Answer

A. Write a balanced chemical reaction for this reaction.

The equation (unbalanced) is:

H2 + N2 = NH3

Let's balance N first, we have 2N atoms on the reactants and 1 on the products, we then add a 2 next to NH3

H2 + N2 = 2NH3

Now, N is balanced, we have 2H on the reactants and 6H on the products, we then add a 3 next to H2 and the balanced equation would be:

3H2 + N2 = 2NH3

B. Given 33.6 g of N2 and 6.0 grams of H2 in a 500mL container.

C. What is the limiting reagent?

According to the balanced chemical equation, we would need 6g H2 (3 moles) for every 28g N2 (1 mole). Since we have 6g H2 in the container and 33.6g N2, we have an excess of N2 and thus H2 is the limiting reagent.

D. Assuming 100% efficiency, how much ammonia would be produced?

We calculate this using the limiting reagent (6g H2):

6g H2 (1 mol H2 / 2g H2) (2 mol NH3 / 3 mol H2) (17g NH3 / 1 mol NH3) = 34g NH3

E. How many grams of each reactant would be left over?

If there was a 100% efficiency, we would only have 33.6g - 28g = 5.6g N2 left

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