As long as there is some oxygen, the reaction will occur. If there is an insufficient amount of oxygen, then the oxygen will be the limiting reacting and there will be excess of the other reactants.
Two changes would make this reaction reactant-favored
C. Increasing the temperature
D. Reducing the pressure
<h3>Further explanation</h3>
Given
Reaction
2H₂ + O₂ ⇒ 2H₂0 + energy
Required
Two changes would make this reaction reactant-favored
Solution
The formation of H₂O is an exothermic reaction (releases heat)
If the system temperature is raised, then the equilibrium reaction will reduce the temperature by shifting the reaction in the direction that requires heat (endotherms). Conversely, if the temperature is lowered, then the equilibrium shifts to a reaction that releases heat (exothermic)
While on the change in pressure, then the addition of pressure, the reaction will shift towards a smaller reaction coefficient
in the above reaction: the number of coefficients on the left is 3 (2 + 1) while the right is 2
As the temperature rises, the equilibrium will shift towards the endothermic reaction, so the reaction shifts to the left towards H₂ + O₂( reactant-favored)
And reducing the pressure, then the reaction shifts to the left H₂ + O₂( reactant-favored)⇒the number of coefficients is greater
Answer:
It all depends what your working with and what experiment your planning on doing .
Explanation:
Say if you were working with chemicals you would the tools that would help you protect your body like gloves,googles, apron , etc
So in conclusion it depends what your doing to know what tools you are going to need
Molar mass Argon = <span>39.948 g/mol
number of moles = mass solute / molar mass
n = 150 / </span><span>39.948
n = 3.7548 moles
hope this helps!</span>
