A gaseous mixture containing 4.15 mol of hydrogen gas and 7.13 mol of oxygen gas reacts to form steam
(a) Write the balanced equation for the reaction.
(b) What is the limiting reactant?
(c) What is the theoretical yiels of steam in moles?
(d) How many moles of the excess reactant remain unreacted?
1. equation
Start with the equation:
2H2+O2 = 2H2O
Since both H2 and O2 are in gaseous forms, the coefficients are in proportion to the volume of the gases.
2. limiting reactant
since the ratio of the volumes of hydrogen and oxygen is 4.15/7.13=0.58 (as opposed to 2/1=2 in the equation), can you determine which gas is the limiting reactant?
3. theoretical yield:
4.15 mol of H2 will react with 2.075 mol of O2. Determine the theoretical yield from the equation in (1).
4. Excess reactant
is what is not being used.
Post your answers for checking if you wish.
(a) The balanced equation for the reaction is:
2H2 + O2 -> 2H2O
(b) To determine the limiting reactant, we compare the amount of each reactant to the stoichiometric ratio in the balanced equation:
From the equation, we can see that for every 2 moles of hydrogen gas (H2), we need 1 mole of oxygen gas (O2).
Given that we have 4.15 moles of hydrogen gas and 7.13 moles of oxygen gas, we can calculate the ratio of the actual amounts of each reactant:
Hydrogen gas: Oxygen gas
4.15 mol: 7.13 mol
To determine the limiting reactant, we need to compare the ratio to the stoichiometric ratio of the balanced equation (2:1):
4.15 mol H2 / 2 = 2.075 mol H2
7.13 mol O2 / 1 = 7.13 mol O2
We can see that the ratio of H2 to O2 is less than the stoichiometric ratio. Therefore, hydrogen gas (H2) is the limiting reactant.
(c) The theoretical yield of steam in moles can be calculated using the stoichiometric ratio from the balanced equation. From the equation, we can see that for every 2 moles of hydrogen gas (H2), we produce 2 moles of water (H2O).
Since hydrogen gas is the limiting reactant, we can determine the moles of steam produced based on the moles of hydrogen gas:
2.075 mol H2 x (2 mol H2O / 2 mol H2) = 2.075 mol H2O
Therefore, the theoretical yield of steam in moles is 2.075 mol.
(d) To determine the moles of the excess reactant remaining unreacted, we can use the stoichiometric ratio from the balanced equation. From the equation, we can see that for every 2 moles of hydrogen gas (H2), we produce 2 moles of water (H2O).
Since hydrogen gas (H2) is the limiting reactant, we can calculate the moles of hydrogen gas that react:
4.15 mol H2 - 2.075 mol H2 = 2.075 mol H2
Therefore, there are 2.075 moles of excess hydrogen gas remaining unreacted.
To answer these questions, we need to go through the problem step by step.
(a) Write the balanced equation for the reaction:
First, we need to determine the balanced equation for the reaction between hydrogen gas (H2) and oxygen gas (O2) to form steam (H2O). The balanced equation is:
2H2 + O2 → 2H2O
(b) Find the limiting reactant:
To determine the limiting reactant, we compare the number of moles of each reactant to the stoichiometric ratio in the balanced equation. In this case, the ratio of H2 to O2 is 2:1. So, for every 2 moles of H2, we need 1 mole of O2 for complete reaction.
For H2, we have 4.15 moles, and for O2, we have 7.13 moles.
Based on the ratio, we can calculate the moles of O2 required:
7.13 moles O2 * (1 mole O2 / 2 moles H2) = 3.565 moles O2
Since we have an excess of O2 (7.13 moles > 3.565 moles), we can conclude that hydrogen gas is the limiting reactant.
(c) Find the theoretical yield of steam in moles:
Now that we know that hydrogen gas is the limiting reactant, we can determine the theoretical yield of steam. According to the balanced equation, 2 moles of H2 react to produce 2 moles of H2O.
Since we have 4.15 moles of H2, the theoretical yield of steam is also 4.15 moles.
(d) Find the moles of excess reactant that remain unreacted:
To find the moles of excess reactant remaining, we need to subtract the amount of the limiting reactant consumed from the initial amount of the excess reactant.
The initial amount of excess O2 is 7.13 moles, but we have determined that only 3.565 moles are needed for complete reaction. Therefore, the excess O2 remaining is:
7.13 moles - 3.565 moles = 3.565 moles
So, 3.565 moles of excess O2 remain unreacted.
To summarize:
(a) The balanced equation for the reaction is: 2H2 + O2 → 2H2O
(b) Hydrogen gas (H2) is the limiting reactant.
(c) The theoretical yield of steam in moles is 4.15 moles.
(d) 3.565 moles of excess O2 remain unreacted.