Ammonia reacts with oxygen gas to form nitrogen monoxide and water. At constant temperture and pressure, how many of nitrogen monoxide can be made by the reaction of 800. ml of oxygen gas?
how many nitrogen monoxide WHAT can be.....
thanks i solved it already
To determine the number of moles of nitrogen monoxide produced by the reaction of 800 mL of oxygen gas, we need to first calculate the number of moles of oxygen gas.
Here's the step-by-step process:
1. Identify the balanced chemical equation for the reaction:
4 NH₃ + 5 O₂ → 4 NO + 6 H₂O
2. Use the ideal gas law equation to calculate the number of moles of oxygen gas (O₂):
PV = nRT
Since the temperature (T) and pressure (P) are constant, we can rewrite the equation as:
V = n(RT/P)
R is the ideal gas constant (0.0821 L·atm/mol·K), T is the temperature in Kelvin, P is the pressure, and V is the volume in liters.
3. Convert the volume of oxygen gas (800 mL) to liters:
800 mL = 800/1000 = 0.8 L
4. Plug the values into the equation:
n = (0.8 L)(R)(T/P)
Here, you will need to provide the temperature and pressure at which the reaction is occurring, so we can calculate the number of moles of oxygen gas.
5. Calculate the number of moles of oxygen gas (n).
6. Finally, use the stoichiometry of the balanced chemical equation to determine the number of moles of nitrogen monoxide formed. According to the equation, 5 moles of oxygen gas produce 4 moles of nitrogen monoxide.
Once you have the number of moles of oxygen gas, multiply it by the appropriate stoichiometric ratio to determine the number of moles of nitrogen monoxide produced.