The number of moles of oxygen (O2) required to completely react with 27.4 mol of H2 is 13.7 moles.
<h3>How to calculate number of moles?</h3>
The number of moles of a substance can be calculated using stoichiometry as follows:
The following balanced chemical equation is given as follows:
2H2 + O2 = 2H2O
According to this question, 2 moles of hydrogen gas (H2) reacts with 1 mole of oxygen gas (O2).
This means that 27.4 moles of hydrogen gas (H2) will react with 27.4/2 = 13.7moles of oxygen gas.
Therefore, the number of moles of oxygen (O2) required to completely react with 27.4 mol of H2 is 13.7 moles.
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Elements 2 and 4 is the answer
Answer:
2193.8 PSI is the pressure in the tank
Explanation:
We apply the Ideal Gases Law to solve this:
P . V = n . R . T
T° is the temperature in K, so we must do the conversion:
35°C + 273 = 308K
P . 1650L = 9750 mol . 0.082 L.atm/mol.K . 308K
P = (9750 mol . 0.082 L.atm/mol.K . 308K) / 1650L → 149.24 atm
Let's make the conversion:
1 atm = 14.7 PSI → 149.24 atm . 14.7 PSI / 1 atm = 2193.8 PSI
And the significant amount of volume can be differed by its solitude
