Refer to the scenario and balanced equation.
2H2 + O2 → 2H2O
At the beginning of the reaction, it is measured that there are 15.0 g of hydrogen (H2) and 97.0 g of oxygen (O2).
What is the theoretical yield for the water that will be produced in the reaction? (M H2O = 18.0 g/mol; M CH4 = 16.0 g/mol)
5.38 x 100 g H2O
1.34 x 102 g H2O
1.08 x 102 g H2O
2.73 x 101 g H2O
PLEASE IM DESPERATE!!!!!
Hydrogen and oxygen can react to form water. This reaction produces a lot of heat energy. 2H2 + O2 → 2H2O While this reaction is thermodynamically feasible (i.e. water has a much lower free energy than the hydrogen/oxygen mixture), there is a large kinetic (activation energy) barrier to the reaction happening.
is what i found to maybe help u its not the answer but itll help
To find the theoretical yield for the water produced in the reaction, we need to determine the limiting reactant.
Step 1: Find the number of moles of each reactant.
First, we convert the masses of hydrogen gas (H2) and oxygen gas (O2) into moles using their molar masses.
Number of moles of H2 = mass of H2 / molar mass of H2
= 15.0 g / (2 g/mol)
= 7.5 mol
Number of moles of O2 = mass of O2 / molar mass of O2
= 97.0 g / (32 g/mol)
= 3.0 mol
Step 2: Determine the molar ratio between the reactants and the product.
From the balanced equation, we see that 2 moles of H2 react with 1 mole of O2 to produce 2 moles of H2O.
Based on the molar ratio, if all the reactants are completely consumed, 2 moles of H2 will require 1 mole of O2.
Step 3: Identify the limiting reactant.
To determine the limiting reactant, compare the moles of reactants with the stoichiometric ratio.
H2:O2 ratio = 2:1
Since we have 7.5 moles of H2 and 3.0 moles of O2, it is clear that we have an excess of H2 and a limiting amount of O2. Therefore, O2 is the limiting reactant.
Step 4: Calculate the theoretical yield.
The theoretical yield is the maximum amount of product that can be formed from the limiting reactant.
From the balanced equation, we see that 1 mole of O2 will produce 2 moles of H2O.
Number of moles of H2O = moles of O2 × (2 moles H2O / 1 mole O2)
= 3.0 mol × (2 mol H2O / 1 mol O2)
= 6.0 mol
Step 5: Convert the moles of H2O to grams.
Using the molar mass of H2O, we can convert the number of moles to grams.
Mass of H2O = number of moles × molar mass
= 6.0 mol × (18.0 g/mol)
= 108.0 g
Therefore, the theoretical yield for the water (H2O) produced in the reaction is 108.0 g H2O.
None of the given answer choices match the calculated value.