What volume of carbon monoxide gas (at STP) is needed when 1.35 Moles of oxygen gas react completely in the following equation. 2CO + O2 > 2CO2 please show your work I'm having trouble with Gas Stoichiometry.
The steps you go through to solve stoichiometry problems.
1. Convert everything to mols.
2. Use the coefficients in the balanced equation to convert what you have to what you want.
3. Convert mols of what you want to other units (grams, liters, kg, etc).
For this problem. We already have mols so you can skip #1.
#2. Use the coefficients in the balanced equation to convert mols O2 (what we have) to mols CO (what we want).
1.35 mol O2 x (2 mol CO/1 mol O2) = 1.35 mol O2 x (2/1) = 2.70 mol O2 needed.
3. Convert 2.70 mol O2 to volume.
2.70 mol x (22.4 L/mol) = 60.48 which rounds to 60.5 L CO needed.
To solve this problem using gas stoichiometry, we need to use the balanced equation and convert moles of oxygen gas (O2) to moles of carbon monoxide gas (CO). Let's go through the steps one by one:
Step 1: Write the balanced equation
The balanced equation given is: 2CO + O2 > 2CO2
Step 2: Determine the mole ratio
From the balanced equation, we can see that 2 moles of carbon monoxide (CO) reacts with 1 mole of oxygen gas (O2) to produce 2 moles of carbon dioxide (CO2). This gives us the mole ratio: 2 CO : 1 O2.
Step 3: Convert moles of oxygen gas to moles of carbon monoxide
Given that we have 1.35 moles of oxygen gas (O2), we can use the mole ratio to find the corresponding moles of carbon monoxide (CO).
1.35 moles O2 * (2 moles CO / 1 mole O2) = 2.7 moles CO
Step 4: Convert moles of carbon monoxide to volume at STP
At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 liters. Therefore, we can convert the moles of carbon monoxide to volume using the following conversion factor:
2.7 moles CO * (22.4 liters / 1 mole CO) = 60.48 liters CO
So, at STP, 1.35 moles of oxygen gas reacts completely to produce 60.48 liters of carbon monoxide gas.