Based on the balanced equation, if 60.1 grams of Nitrogen (N2) are used, how many grams of ammonia (NH3) is made? 3 H2 + 1 N2 > 2 NH3

73.07 grams of ammonia is produced.

Explanation:

In order to find the grams of ammonia produced, we need to find the amount of the reactants so that we know how much product (ammonia) the reactants (Hydrogen and Nitrogen) can and will produce.

First, we need to use the balanced equation to find the amount of moles equivalent to the 60.1 grams of Nitrogen that reacts.

To convert from Grams to Moles, we will divide by the molar mass (amu)..

60.1 grams of N2 /  2(14.01) grams  N2 = 2.144896502 moles of N2.

So, we know that 60.1 grams of N2 equals 2.144896502 moles.

       Now, we will look at the balanced equation and convert from moles of N2 to moles of NH3 in order to later find the grams of NH3 (ammonia) produced..

2.144896502 moles N2 *  2 moles NH3/1 mol N2 = 4.289793004 moles NH3.

     Now that we know the amount of moles produced of ammonia, we will convert to grams. We can do this by multiplying by the molar mass of ammonia which is 17.034 (N = 14.01, H = 1.008, ---> 14.01 +3(1.008) = 17.034)

4.289793004 moles NH3 * 17.034/1 mol = 73.07233403 grams NH3

This can be estimated to 73.07 grams of NH3 (ammonia) produced.

If you are still confused on how to convert between moles and grams, please see the uploaded image.

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in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

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