Question #1efb5
1 Answer
!! LONG ANSWER !!
Like always, start with the balanced chemical equation
This first thing you must do is have a good look at the mole ratios that exist between all the species involved in the reaction. Notice that you need 3 moles of hydrogen gas to react with 1 mole of nitrogen gas in order to produce 2 moles of ammonia.
These ratios are the key to this problem. So, you know that, when 12.3 g of hydrogen react with excess nitrogen, 55.8 g of ammonia are formed.
You need to check to see what the percent yield of this reaction is, i.e. how much of the reactants are turned into the product.
The number of moles of hydrogen that reacted is
According to the
However, the reaction actually produced
This means that, as suspected, your reaction does not have a 100% yield; the actual yield is
The percent yield of the reaction is very important because it will tell you exactly how much ammonia will be produced when 280.2 g of nitrogen react with excess hydrogen.
This time, the number of moles of nitrogen that react will be
According to the
But since the reaction's percent yield is not 100%, but actually 80.7%, that much nitrogen will produce
Use ammonia's molar mass to determine the mass produced
Since you know the temperature (I won't write the conversion to Kelvin since the answer is quite long already), volume, and number of moles, you can use the ideal gas law equation to solve for the system's pressure
Rounded to three sig figs, the answer will be