Consider the reaction,
4 NH3 + 5 O2 => 4 NO + 6 H2O
How many grams of NO will be made from 10.7 moles of O2?
Look at your stoichiometry problems. This is just another stoiciometry problem.
To find the number of grams of NO produced from a given amount of O2, we need to use the molar ratio between O2 and NO in the balanced chemical equation.
Let's start by calculating the molar mass of NO. The molar mass of nitrogen (N) is 14.01 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol. Since NO consists of one nitrogen atom and one oxygen atom, its molar mass is 14.01 + 16.00 = 30.01 g/mol.
Now, we can use the balanced chemical equation to determine the molar ratio between O2 and NO. From the equation, we can see that 5 moles of O2 react to produce 4 moles of NO.
Next, we use the given number of moles of O2 and the molar ratio to find the number of moles of NO produced. The equation is:
10.7 moles O2 x (4 moles NO / 5 moles O2) = 8.56 moles NO
Finally, we can convert the moles of NO to grams using the molar mass of NO:
8.56 moles NO x (30.01 g NO / 1 mole NO) = 257.57 grams NO
Therefore, 10.7 moles of O2 will produce 257.57 grams of NO.