Calculate the concentration of CO 2 in orange soda
that
was bottled (at a certain temperature) with a partial pressure of
CO 2 of 3.15 atm over the
liquid.
At that temperature, the Henry's law constant, k, for CO
2 is 3.05 x 10 -2
mol/L atm.
(i.e., 3.05 x 10 -2
M/atm)
14.0 M |
||
8.12 M |
||
2.74 M |
||
6.63 x 10 -3 M |
||
0.0961 M |
||
23.8 M |
||
11.9 M |
||
7.93 x 10 -1 |
2.
What is the mole fraction of sucrose when 433 g sucrose C 12H 22O 11 (molar mass 342.3 g/mol) is dissolved in 655 g water?
0.0336 |
||
0.101 |
||
0.0456 |
||
1.03 |
||
1.75 |
3.
A bottle of orange beverage has CO 2 concentration
equal to 0.0801 Molar at a certain temperature. What is the partial
pressure of CO 2 in the container above the liquid in
atm?
At this temperature, the Henry's law constant, k, for CO
2 is 3.60 x 10 -2
mol/L atm. (i.e., 3.20 x 10
-2 M/atm)
0.842 atm |
||
5.28 atm |
||
1.55 x 10-1 atm |
||
3.20 x 10-3 atm |
||
0.422 atm |
||
2.23 atm |
||
4.51 atm |
||
2.98 atm |
Answer:-
(1)-
Given:-
partial pressure of CO2 (p) = 3.15 atm
Henry's law constant (k) for CO2 = 3.05 10-2 mol / L atm = 3.05 10-2 M / atm
concentration of CO2 (c) = ?
As we know that according to the Henry's Law , the mass of a gas dissolved per unit volume of a solvent i.e concentration (c) is directly proportional to the partial pressure (p) of the gas in equilibrium with the solution at a given temperature.
So
concentration of a gas (c) partial pressure (p) of the gas
then
concentration of a gas (c) = Henry's law constant (k) partial pressure (p) of the gas
therefore
concentration of a CO2 gas (c) = Henry's law constant (k) of CO2 gas partial pressure (p) of the CO2 gas
concentration of a CO2 gas (c) = 3.05 10-2 M / atm 3.15 atm
concentration of a CO2 gas (c) = 9.61 10-2 M
concentration of a CO2 gas (c) = 0.0961 M (i.e the answer)
(2)-
Given:-
wt. of sucrose (C12H22O11) i.e (wsucrose) = 433 g
molar mass of sucrose (C12H22O11) i.e (Msucrose) = 342.3 g/mol
wt. of water (H2O) i.e (wwater) = 655 g
Since we know that
molar mass of water (H2O) i.e (Mwater) = 18 g/mol
As we know that
no. of moles of compound (ncompound) = wt. of compound (wcompound) / molar mass of compound (Mcompound)
therefore
no. of moles of compound (nsucrose) = wt. of compound (wsucrose) / molar mass of compound (Msucrose)
no. of moles of compound (nsucrose) = 433 g / 342.3 g/mol
no. of moles of compound (nsucrose) = 1.26 mol
similarly
no. of moles of compound (nwater) = wt. of compound (wwater) / molar mass of compound (Mwater)
no. of moles of compound (nwater) = 655 g / 18 g/mol
no. of moles of compound (nwater) = 36.39 mol
Also we know that
total no. of moles in solution (ntotal) = no. of moles of compound (nsucrose) + no. of moles of compound (nwater)
total no. of moles in solution (ntotal) = 1.26 mol + 36.39 mol
total no. of moles in solution (ntotal) = 37.65 mol
So according to the formula
mole fraction of sucrose (C12H22O11) i.e (sucrose) = no. of moles of compound (nsucrose) / total no. of moles in solution (ntotal)
mole fraction of sucrose (C12H22O11) i.e (sucrose) = 1.26 mol / 37.65 mol
mole fraction of sucrose (C12H22O11) i.e (sucrose) = 0.0335 (i.e the answer)
(3)-
Given:-
Henry's law constant (k) for CO2 = 3.60 10-2 mol / L atm = 3.60 10-2 M / atm
concentration of CO2 (c) = 0.0801 M
partial pressure of CO2 (p) = ?
As we know that
concentration of a gas (c) = Henry's law constant (k) partial pressure (p) of the gas
therefore
0.0801 M = 3.60 10-2 M / atm partial pressure (p) of the CO2 gas
partial pressure (p) of the CO2 gas = 0.0801 M / 3.60 10-2 M / atm
partial pressure (p) of the CO2 gas = 0.0801102 atm / 3.60
partial pressure (p) of the CO2 gas = 0.0223 102 atm
partial pressure (p) of the CO2 gas = 0.0223 100 atm
partial pressure (p) of the CO2 gas = 2.23 atm (i.e the answer)
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