Consider this equilibrium:
2 answers:
Answer:
It decreases as the concentration of products decreases.
It increases as the concentration of products increases.
Explanation:
the equilibrium reaction is
As per equilibrium,
a) there will be no effect of pressure change on the equilibrium as the number of gaseous molecules are same on both the side of reaction.
b) there will be no effect of addition of inert gas on the equilibrium as the number of gaseous molecules are same on both the side of reaction.
c) the reverse reaction rate can be increased by
i) decreasing the concentration of reactants
ii) increasing the concentration of products
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Answer:
The Experimental Molar Volume in L/mol of the Hydrogen gas=23.36L/mol
Explanation:
We are given that
Volume of H2 at STP=52.8mL
Mass of magnesium metal ,M(Mg)=0.055g
We have to find the Experimental Molar Volume in L/mol of the Hydrogen gas.
Molar mass of Mg=24.305 g/mol
Number of moles=
Using the formula
Number of moles of Mg=moles
Number of moles of Mg=0.00226moles
Number of moles of Mg=Number of moles of H2
Number of moles of H2=0.00226moles
Molar volume of Hydrogen gas (H2)=
Molar volume of Hydrogen gas (H2)=
Molar volume of Hydrogen gas (H2)=
Molar volume of Hydrogen gas (H2)=23.36L/mol
Hence, the Experimental Molar Volume in L/mol of the Hydrogen gas=23.36L/mol