N2(g) + O2(g) → N2O5(g)
What volume of oxygen gas reacts to yield 750.0 cm3 of N2O5? The reaction conditions are 350°C and 2.50 atm pressure.
2N2 + 5 O2 = 2N2O5 I balanced correctly. What is my next step to solve this problem. I am confused and I want to understand the steps. Thank you.
Stoichiometry by any other name is stoichiometry. Since all are gases and the conditions apply to everything you can use the shortcut.
750 cc N2O5 x (5 mol O2/2 mols N2O5) = 750 cc (5/2) = ?
To solve the problem, you can use the ideal gas law equation, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
1. Convert the given volume of N2O5 from cm3 to liters:
750.0 cm3 = 750.0 cm3 * (1 L / 1000 cm3) = 0.750 L
2. Convert the given temperature from Celsius to Kelvin:
Temperature in Kelvin = 350°C + 273.15 = 623.15 K
3. Determine the number of moles of N2O5 using the ideal gas law equation:
PV = nRT
(2.50 atm) * (0.750 L) = n * (0.0821 L-atm/mol-K) * (623.15 K)
n = (2.50 atm * 0.750 L) / (0.0821 L-atm/mol-K * 623.15 K)
4. Calculate the number of moles of oxygen gas (O2) using the balanced equation:
From the balanced chemical equation, we know that 5 moles of O2 react to produce 2 moles of N2O5.
Therefore, the number of moles of O2 = (n moles of N2O5) * (5 mol O2 / 2 mol N2O5)
5. Finally, calculate the volume of oxygen gas (O2) in cm3:
Volume of O2 = (number of moles of O2) * (22.4 L/mol) * (1000 cm3 / 1 L)
By following these steps, you will be able to determine the volume of oxygen gas required to yield 750.0 cm3 of N2O5 under the given reaction conditions.