I took this I believe it’s A
You will need 1 moles. Hope this helps!!
Answer:
Mass of Cu(NO₃)₂ produced = 125.67 g
limiting reactant = Cu
Explanation:
Given data:
Mass of Cu = 42.6 g
Mass of HNO₃ = 84.0 g
What is limiting reactant = ?
Mass of Cu(NO₃)₂ produced = ?
Solution:
Chemical equation:
3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 4H₂O + 2NO
Number of moles of Cu:
Number of moles = mass/ molar mass
Number of moles = 42.6 g/63.546 g/mol
Number of moles = 0.67 mol
Number of moles of HNO₃:
Number of moles = mass/ molar mass
Number of moles = 84 g/63.01 g/mol
Number of moles = 1.3 mol
Now we will compare the moles of Cu(NO₃)₂ with HNO₃ and Cu from balance chemical equation.
HNO₃ : Cu(NO₃)₂
8 : 3
1.3 : 3/8×1.3 = 6
Cu : Cu(NO₃)₂
3 : 3
0.67 : 0.67
Number of moles of Cu(NO₃)₂ produced by Cu are less so Cu will limiting reactant.
Mass of Cu(NO₃)₂:
Mass = number of moles × molar mass
Mass = 0.67 mol × 187.56 g/mol
Mass = 125.67 g
Answer : The correct expression for equilibrium constant will be,
Explanation :
Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.
The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.
As we know that the concentrations of pure solids and liquids are constant that is they do not change. Thus, they are not included in the equilibrium expression.
The given equilibrium reaction is,
The expression of will be,
Therefore, the correct expression for equilibrium constant will be,
Answer:
Equilibrium constant of the given reaction is
Explanation:
....
....
The given reaction can be written as summation of the following reaction-
......................................................................................
Equilibrium constant of this reaction is given as-