According to the balanced chemical equation, 3 moles of oxygen gas (O2) are needed to produce 2 moles of dinitrogen trioxide (N2O3).
Since we have 15.0 liters of dinitrogen trioxide (N2O3), we first need to convert this volume to moles using the ideal gas law:
PV = nRT
where:
P = pressure (assume constant)
V = volume (15.0 liters)
n = moles
R = ideal gas constant
T = temperature (assume constant)
Next, we can use the mole ratio from the balanced chemical equation to calculate the moles of oxygen gas (O2) needed and then convert this to liters using the ideal gas law.
Using this information, we can calculate the number of liters of oxygen gas needed to produce 15.0 liters of dinitrogen trioxide.
Calculate the number of liters of oxygen gas needed to produce 15.0 liters of dinitrogen trioxide. Assume all gases are at the same conditions of temperature and pressure.
2N2(g) + 3O2(g) → 2N2O3(g
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