determine the volume of the residual gas at 20.0cm³ of hydrogen was sparked with 15.0cm³ of oxygen and the resulting mixture cooled at room temperature
2H2 + O2 ==> 2H2O
The coefficients tell you 2 mols H2 will use 1 mol O2 or
20 cc H2 will use 10 cc O2. So how much O2 remains?
Well, it seems like we have a chemistry question here! Let me think... Oxygen and hydrogen? That sounds like a recipe for a little fire dance, doesn't it?
So, when these two gases react, they form water (H2O). And water is not a gas, it's a liquid! So we won't be dealing with gases anymore, but with liquids.
To determine the volume of the residual gas, we need to know what gas is left after the reaction. But in this case, since we're forming liquid water, there won't be any residual gas.
So, the volume of the residual gas would be zero! It's like the gases partied a little too hard and disappeared completely. Better luck next time, gases!
To determine the volume of the residual gas, we need to first calculate the volume of hydrogen and oxygen that react to form water.
1. Convert the volumes of hydrogen and oxygen to moles using the ideal gas law equation:
n = PV / RT
For hydrogen:
P₁ = pressure of hydrogen (assumed to be constant)
V₁ = volume of hydrogen = 20.0 cm³
T₁ = temperature of hydrogen (assumed to be constant)
R = ideal gas constant (0.0821 L·atm/mol·K)
For oxygen:
P₂ = pressure of oxygen (assumed to be constant)
V₂ = volume of oxygen = 15.0 cm³
T₂ = temperature of oxygen (assumed to be constant)
Let's assume the pressure, temperature, and amount of gas are the same for the reactants and products.
2. Determine the balanced chemical equation for the reaction between hydrogen and oxygen to form water:
2H₂(g) + O₂(g) → 2H₂O(g)
According to the stoichiometry of the reaction, 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.
3. Determine the limiting reactant:
Compare the calculated moles of hydrogen and oxygen to determine which is the limiting reactant (i.e., the reactant that completely consumes the other reactant).
4. Calculate the moles of water produced:
Since the stoichiometry of the reaction shows that 2 moles of water are produced for every 2 moles of hydrogen reacted, the moles of water will be the same as the moles of hydrogen reacted.
5. Calculate the volume of the residual gas (water):
We need to determine the volume of the water formed using the ideal gas law equation:
V = nRT / P
For water (residual gas):
P = pressure of the water (assumed to be constant)
n = number of moles of water produced
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature of the water (assumed to be ambient temperature)
By following these steps, you can calculate the volume of the residual gas (water) formed in the reaction.
To determine the volume of the residual gas, we need to understand the chemical reaction that occurred between hydrogen and oxygen. In this case, the reaction results in the formation of water (H2O), so there should be no residual hydrogen or oxygen gas left.
The reaction equation for the combination of hydrogen and oxygen to form water is:
2H2 + O2 → 2H2O
This equation tells us that 2 moles of hydrogen gas (H2) react with 1 mole of oxygen gas (O2) to form 2 moles of water (H2O).
To find the volume of the residual gas, follow these steps:
Step 1: Determine the moles of hydrogen and oxygen used.
Given that the initial volumes of hydrogen and oxygen are 20.0 cm³ and 15.0 cm³ respectively, we can assume the gases were at room temperature and at the same pressure. We can use the ideal gas law to find the moles of hydrogen and oxygen.
PV = nRT
Where:
P = pressure (assumed constant)
V = volume
n = number of moles
R = ideal gas constant
T = temperature (assumed constant)
Since the pressure, temperature, and volume are constant, we can simplify the equation to:
n = PV / RT
We will need to know the pressure and temperature to calculate the moles accurately.
Step 2: Determine the moles of water formed.
Based on the balanced chemical equation 2H2 + O2 → 2H2O, we know that for every 2 moles of hydrogen used (or 1 mole of oxygen used), 2 moles of water are formed.
Step 3: Calculate the volume of residual gas.
If the reaction went to completion and no residual hydrogen or oxygen was left, this means all the hydrogen and oxygen reacted to form water. Therefore, the volume of the residual gas would be zero.
Please note that if there was an incomplete reaction or some other factors affecting the reaction, the above calculation might not be applicable. In such cases, additional information might be needed to accurately determine the volume of the residual gas.