Consider the reaction
4KO2(s) + 2CO2(g) !
2K2CO3(s) + 3O2(g) .
How much KO2 is needed to react with 75.0 L
of carbon dioxide at STP?
Well, according to the balanced equation, for every 2 moles of KO2, we need 1 mole of CO2. And at STP, 1 mole of any gas occupies 22.4 L. So, let's do some math! If 22.4 L of CO2 requires 2 moles of KO2, then 75.0 L of CO2 would require (2/22.4) x 75.0 moles of KO2. That's about 6.70 moles of KO2. So, you would need approximately 6.70 moles of KO2 to react with 75.0 L of CO2 at STP. Just remember, the actual reaction is not as "KO2-l" as this answer!
To determine how much KO2 is needed to react with 75.0 L of carbon dioxide at STP, we need to use the given balanced chemical equation and molar volume at STP.
1. First, let's determine the molar volume of a gas at STP:
- The molar volume of a gas at STP is equal to 22.4 L/mol.
2. Now, let's calculate the number of moles of carbon dioxide:
- Given volume of carbon dioxide = 75.0 L
- Using the molar volume at STP: 75.0 L / 22.4 L/mol = 3.35 moles of CO2
3. Next, let's use the stoichiometry of the balanced chemical equation to determine the moles of KO2 required:
- From the balanced equation: 4 moles KO2 reacts with 2 moles CO2
- So, 2 moles of CO2 will react with 4/2 = 2 moles of KO2
4. Now, let's calculate the moles of KO2 needed:
- Moles of KO2 = 2 moles of CO2 x (2 moles KO2 / 2 moles CO2) = 2 moles of KO2
Therefore, you would need 2 moles of KO2 to react with 75.0 L of carbon dioxide at STP.
To find out how much KO2 is needed to react with 75.0 L of carbon dioxide at STP (Standard Temperature and Pressure), we need to use stoichiometry, which relates the amount of reactants and products in a chemical equation.
First, let's look at the balanced chemical equation:
4KO2(s) + 2CO2(g) → 2K2CO3(s) + 3O2(g).
From the balanced equation, we can see that 4 moles of KO2 react with 2 moles of CO2. This means the stoichiometric ratio between KO2 and CO2 is 4:2, which simplifies to 2:1.
To find the amount of KO2 needed, we'll follow these steps:
Step 1: Convert the given volume of CO2 to moles using the ideal gas law equation PV = nRT.
PV = nRT,
n = (PV) / (RT),
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
At STP, the temperature (T) is 273.15 K and the pressure (P) is 1 atm.
n = [(1 atm) × (75.0 L)] / [(0.0821 L·atm/mol·K) × (273.15 K)]
n ≈ 2.84 moles
Step 2: Use the stoichiometric ratio to determine the amount of KO2 needed.
According to the stoichiometry, for every 2 moles of CO2, 4 moles of KO2 are required in the reaction.
So, for 2.84 moles of CO2, we can calculate the amount of KO2 needed:
(4 moles KO2 / 2 moles CO2) × (2.84 moles CO2) = 5.68 moles KO2
Therefore, approximately 5.68 moles of KO2 are needed to react with 75.0 L of carbon dioxide at STP.
You need to find the arrow key on your computer and use it. ==> or --> but not !.
Convert 75.0L CO2 to mols. mols = L/22.4 = ?
Use the coefficients in the balanced equation to convert mols CO2 to mols KO2.
Then g KO2 = mols x molar mass.