Given the following equation: NH3 + NH3 +O2 �¨ NO + H2O
Calculate the number of grams of ammonia needed to form 40.12 moles of nitrogen monoxide.
a. You need to make sure the equation is correct. Do you really need to write NH3 twice or is that a typo? Second, you mut balance the equation.
The matter of solving it is stoichiometry. Here is an exmple of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
does that work the same way with moles
Does WHAT work the same way with moles. The instructions for the stoichiometry problem converts everything to moles FIRST, then uses the equation to convert moles of one substance to moles of another substance. So for your problem, step 1 (convert grams to moles) has been done already and you don't need to do that step.
To calculate the number of grams of ammonia needed to form 40.12 moles of nitrogen monoxide, we need to use stoichiometry.
The balanced equation for the reaction is:
2NH3 + O2 --> 2NO + 3H2O
From the balanced equation, we can see that 2 moles of ammonia react to produce 2 moles of nitrogen monoxide.
So, the molar ratio is 2 moles of NH3 : 2 moles of NO.
To convert moles of nitrogen monoxide to moles of ammonia, we can use the molar ratio:
40.12 moles of NO * (2 moles of NH3 / 2 moles of NO) = 40.12 moles of NH3
Now, to calculate the grams of ammonia, we need to use the molar mass of ammonia (NH3). The molar mass of NH3 is calculated as:
Molar mass(N) + 3 * Molar mass(H) = 14.01 g/mol + 3 * 1.01 g/mol = 17.03 g/mol
Therefore, the grams of ammonia needed can be calculated as:
40.12 moles of NH3 * 17.03 g/mol = 682.6456 grams of NH3
So, approximately 682.65 grams of ammonia are needed to form 40.12 moles of nitrogen monoxide.