4NH3+5O2--->4NO+6H2O
determine the amount of oxygen needed to produce 1.2x10^4mol of nitrogen monoxide gas
5 moles
To determine the amount of oxygen needed to produce 1.2x10^4 moles of nitrogen monoxide (NO) gas, we need to analyze the balanced chemical equation:
4NH3 + 5O2 ---> 4NO + 6H2O
From the equation, we can see that the molar ratio between O2 and NO is 5:4. This means that for every 5 moles of O2, we can produce 4 moles of NO.
Now, we can set up a proportion to find the amount of O2 needed:
5 moles O2 / 4 moles NO = x moles O2 / 1.2x10^4 moles NO
Cross-multiplying, we get:
5 moles O2 * 1.2x10^4 moles NO = 4 moles NO * x moles O2
Rearranging the equation, we can solve for x:
x = (5 moles O2 * 1.2x10^4 moles NO) / 4 moles NO
x = 6x10^4 moles O2 / 4
x = 15x10^3 moles O2
Therefore, the amount of oxygen needed to produce 1.2x10^4 moles of nitrogen monoxide gas is 15x10^3 moles O2.