# Problem: Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation:N2 (g) + 3 H 2 (g) → 2 NH 3 (g)Given a mixture of 1.00 x 10 3 g N2 and 5.00 x 10 2 g H2, what mass of which starting material would remain unreacted?

###### FREE Expert Solution

Step 1: From the problem, the given combustion reaction is:

N2 (g) + 3 H 2 (g) → 2 NH 3 (g)

Now that we have a balanced equation, we can proceed with the problem.

Step 2: Notice that we are given the mass of both reactants: this means we need to determine the limiting reactant, which is the reactant that forms the less amount of product

This is because once the limiting reactant is all used up, the reaction can no longer proceed and make more products.

This means the limiting reactant determines the maximum mass of the product formed.

We need to perform a mole-to-mole comparison between each reactant and NH3

From N2:

molar mass N2 = 28.02 g/mol

molar mass NH3 = 17.034 g/mol

mass NH3 = 1215.8 g NH3

From H2:

mass NH3 = 2816.5 g NH3

Since N2 forms fewer NH3  → 2 is the limiting reactant.

85% (295 ratings) ###### Problem Details

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation:

N2 (g) + 3 H 2 (g) → 2 NH 3 (g)

Given a mixture of 1.00 x 10 3 g N2 and 5.00 x 10 2 g H2, what mass of which starting material would remain unreacted?

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Based on our data, we think this problem is relevant for Professor Sharma's class at Kean University.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.