The volume of oxygen required to react with 3.2 * 10²² molecules of hydrogen is 0.56 L.
<h3>What is stoichiometric law?</h3>
The stoichiometric law has been given as the representation of the moles of product and reactant in a chemical reaction are represented by the stoichiometric coefficient.
It has been known that 1 mole of a compound has 6.023 * 10²³ molecules. Thus, the moles of hydrogen gas equivalent to 3.2 * 10²² molecules has been:
6.023 * 10²³ molecules = 1 mole
3.2 * 10²² molecules = 1/6.023 * 10²³ * 3.2 * 10²² moles
3.2 * 10²² molecules = 0.05 moles
Thus, the moles of hydrogen gas available is 0.05 moles.
From the stoichiometric law, according to the balanced chemical equation,
2 moles of hydrogen requires = 1 moles of oxygen
0.05 moles of hydrogen requires = 1/2 * 0.05 moles oxygen
0.05 moles of hydrogen requires = 0.025 moles oxygen
Thus, the moles of oxygen required is 0.025 moles. At STP, a mole of gas been equivalent to 22.4 L . Thus, the volume of 0.025 moles oxygen has been:
1 mole = 22.4 L
0.025 moles = 22.4 * 0.025 L
0.025 mole = 0.56 L
Thus, the volume of oxygen required to react with 3.2 * 10²² molecules of hydrogen is 0.56 L.
Learn more about stoichiometric law, here:
brainly.com/question/23742235
#SPJ1
is the amount of heat supplied.
is the mass of the sample.
is the increase in temperature.