Answer:
3) The relative concentrations of each gas must remain constant.
4)The concentration of each gas will not change.
Explanation:
- For the equilibrium system:
<em>X₂ + Y₂ ⇄ 2XY,</em>
The no. of moles of gases in each side is constant; there is 2 moles of gases at reactants side and 2 moles of gases at products side.
So, changing the volume will not affect on the equilibrium system.
<em>So, the right choice is:</em>
3) The relative concentrations of each gas must remain constant.
4)The concentration of each gas will not change.
Explanation:
Transfer of mass A into stagnant film B depends on the availability of driving force.
Whereas driving force is the pressure difference at the surface of A and the bulk.
As, 
Therefore, putting the given values into the above formula as follows.
= 
= 0.132 
Thus, we can conclude that the flux of A from a surface into a mixture of A and B is 0.132
Answer:
B
Explanation:
Oil > Animals > Plants > Chemicals
The new concentrations of 
and 
are 0.25M and 19M
Calculation of number of moles of each component,
Molarity of = number of moles/volume in lit = 0. 500 M
Number of moles = molarity of × volume in lit = 0. 500 M× 0.025 L
Number of moles of = 0.0125 mole
Molarity of = number of moles/volume in lit = 0. 38 M
Number of moles = molarity of × volume in lit = 0. 38 M× 0.025 L
Number of moles of = 0.95 mole
Calculation of new concentration at volume 50 ml ( 0.05L)
Molarity of = number of moles/volume in lit = 0.0125 mole/0.05L
Molarity of = 0.25M
Molarity of = number of moles/volume in lit = 0.95mole/0.05L
Molarity of = 19 M
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Answer:
Explanation:
<u>1) Data:</u>
a) V = 93.90 ml
b) T = 28°C
c) P₁ = 744 mmHg
d) P₂ = 28.25 mmHg
d) n = ?
<u>2) Conversion of units</u>
a) V = 93.90 ml × 1.000 liter / 1,000 ml = 0.09390 liter
b) T = 28°C = 28 + 273.15 K = 301.15 K
c) P₁ = 744 mmHg × 1 atm / 760 mmHg = 0.9789 atm
d) P₂ = 28.5 mmHg × 1 atm / 760 mmHg = 0.0375 atm
<u>3) Chemical principles and formulae</u>
a) The total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas. Hence, the partical pressure of the hydrogen gas collected is equal to the total pressure less the vapor pressure of water.
b) Ideal gas equation: pV = nRT
<u>4) Solution:</u>
a) Partial pressure of hydrogen gas: 0.9789 atm - 0.0375 atm = 0.9414 atm
b) Moles of hygrogen gas:
pV = nRT ⇒ n = pV / (RT) =
n = (0.9414 atm × 0.09390 liter) / (0.0821 atm-liter /K-mol × 301.15K) =
n = 0.00358 mol (which is rounded to 3 significant figures) ← answer
