How many moles of oxygen (O2) are required to completely react with 27.4 mol of H2?
2H2 + O2 ==> 2H2O
Use the coefficients to calculate this.
27.4 mols H2 x (1 mol O2/2 mols H2) = 27.4 x 1/2 = ?
To determine the number of moles of oxygen (O2) required to react with 27.4 mol of H2, we need to consider the balanced chemical equation for the reaction. In this case, the balanced equation is:
2H2 + O2 -> 2H2O
From the equation, we can see that 2 moles of H2 react with 1 mole of O2 to produce 2 moles of H2O. Therefore, the mole ratio between H2 and O2 is 2:1.
To find the number of moles of O2 required, we can use the mole ratio and set up a proportion:
2 mol H2 / 1 mol O2 = 27.4 mol H2 / x mol O2
Cross-multiplying, we have:
2 mol H2 * x mol O2 = 27.4 mol H2 * 1 mol O2
Simplifying the equation, we get:
2x = 27.4
Dividing both sides by 2:
x = 27.4 / 2
Calculating the value:
x = 13.7
Therefore, 13.7 moles of O2 are required to completely react with 27.4 moles of H2.
To determine the number of moles of oxygen (O2) required to react with a given amount of hydrogen (H2), we need to use the balanced chemical equation for the reaction between hydrogen and oxygen.
The balanced chemical equation for the reaction between hydrogen and oxygen is:
2H2 + O2 → 2H2O
From the balanced equation, we can see that 2 moles of H2 react with 1 mole of O2 to produce 2 moles of H2O.
So, for every 2 moles of H2, we need 1 mole of O2.
Given that we have 27.4 moles of H2, we can use this information to calculate the number of moles of O2 required.
Number of moles of O2 = (27.4 mol H2) / (2 mol H2/1 mol O2)
= 13.7 mol O2
Therefore, to completely react with 27.4 moles of H2, we would need 13.7 moles of O2.