16) Acculturation refers to
1 answer:
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Answer:
A) The partial presssure of CO₂ is 167 mm Hg
B) The partial presssure of N₂ is 354 mm Hg
C) The partial presssure of Ar is 235 mm Hg
D) The partial presssure of H₂ is 86 mm Hg
Explanation:
Dalton's law of partial pressures is basically expressed by the following statement:
The total pressure of a mixture is equal to the sum of the partial pressures of its components.
So initially we have:
= total presure of the system (675 mm Hg).
= partial pressure of N₂ (354 mm Hg).
= partial pressure of Ar (235 mm Hg).
Using Dalton's law we can find the partial pressure of H₂:
675 mm Hg=354 mm Hg + 235 mm Hg +
= 675 mm Hg - 354 mm Hg - 235 mm Hg
=86 mm Hg
If CO₂ gas is added to the mixture, at constant temperature, and the volume is the same, the difference between the new total pressure and the previous total pressure is equal to the partial pressure of CO₂.
842 mm Hg= 354 mm Hg + 235 mm Hg + 86 mm Hg +
= 842 mm Hg - 354 mm Hg - 235 mm Hg - 86 mm Hg
= 167 mm Hg
Answer:
Explanation:
Several rules should be followed to write any equilibrium expression properly. In the context of this problem, we're dealing with an aqueous equilibrium:
- an equilibrium constant is, first of all, a fraction;
- in the numerator of the fraction, we have a product of the concentrations of our products (right-hand side of the equation);
- in the denominator of the fraction, we have a product of the concentrations of our reactants (left-hand side o the equation);
- each concentration should be raised to the power of the coefficient in the balanced chemical equation;
- only aqueous species and gases are included in the equilibrium constant, solids and liquids are omitted.
Following the guidelines, we will omit liquid water and we will include all the other species in the constant. Each coefficient in the balanced equation is '1', so no powers required. Multiply the concentrations of the two products and divide by the concentration of carbonic acid: