🤓 Based on our data, we think this question is relevant for Professor Delgado's class at FIU.
Calculate the initial moles of each reactant:
STP: P = 1 atm, T = 0°C (273.15 K)
nCH4 = 7.1382x10-3 mol
nO2 = 0.03925 mol
nNO = 2.5653x10-3 mol
From the balanced reaction 1 mol of CH4(g) react with 5 moles of O2(g) and 5 moles of NO(g)
Divide to moles of O2(g) and moles of NO(g) for stoichiometry:
moles O2 = 7.852x10-3 mol
moles NO = 5.1305x10-4 mol
NO(g) → limiting reactant → will be consumed totally, but only 92.0% reacted
moles NO(g) reacted = (92.0%) (2.5653x10-3 mol)
moles NO(g) reacted = 2.36x10-3 mol
moles CH4(g) left = 7.1382x10-3 mol - (2.36x10-3 mol/5)
moles CH4(g) left = 7.1382x10-3 mol - 4.72x10-4 mol
moles CH4(g) left = 6.66x10-3 mol
moles O2(g) left = 0.03925 mol - 2.36x10-3 mol
moles O2(g) left = 0.0369 mol
moles NO(g) left = 2.5653x10-3 mol - 2.36x10-3 mol
moles NO(g) left = 2.05x10-3 mol
Calculate pressure using the ideal gas equation:
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Delgado's class at FIU.