The answer should be metallic
At STP condition 1 mol of any ideal gas will have a volume of 22.4L
1.75 mol of F2 x 22.4 L / 1 mol = 39.2 L
Percentage yield = (actual yield / theoretical
yield) x 100%<span>
The balanced equation for the reaction is,
CH₄(g) + Cl₂<span>(g) </span>→ CH₃Cl(g)
+ HCl(g)</span><span>
Since there is excess of Cl₂ gas, we can assume that all of CH₄ gas are reacted.</span><span>
Moles of CH₄(g) = mass / molar mass</span><span>
= 25.0 g / 16 g/mol
= 1.5625 mol
The stoichiometric ratio between CH₄(g) and CH₃Cl(g)
is 1 : 1</span><span>
Hence moles of CH₃Cl(g) = 1.5625 mol</span><span>
Molar mass of CH₃Cl(g) = 50.5 g/mol</span><span>
Mass of CH₃Cl(g) = number of moles x molar mass</span><span>
= 1.5625 mol x 50.5 g/mol
<span>
= 78.9 g</span>
Hence theoretical yield = 78.9 g
Actual yield = 45.0 g
Hence,
<span> Percentage yield = (45.0 g / 78.9 g) x 100% </span>
<span>
= 57.03%</span></span>
<span>They keep the same form no matter what tense is used.
</span>
Explanation:
A chemical equilibrium is defined as the state of reaction in which the rate of forward reaction is equal to the rate of backward reaction.
When Q > 
, then it means that the reaction is proceeding in the backward reaction. Whereas if Q < , then it means that the reaction is proceeding in the forward direction. Hence, formation of products will be favored.
On the other hand, if Q = , then it means reaction is at equilibrium.
At equilibrium, it is not necessary that the concentrations of products divided by the concentrations of reactants equals one.
Thus, we can conclude that the statement for a chemical system at equilibrium, the forward and reverse rates of reaction are equal, is correct.
