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The vapor pressure of the solvent decreased by 10 mm Hg, when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the mole fraction of the solvent, if the decrease in vapor pressure of the solvent is required to be 20 mm Hg.?
A
0.2
B
0.1
C
0.4
D
0.6
Correct Answer:
0.6
A very dilute solution is prepared by dissolving 'x
1
' mole of solute in 'x
2
' mole of a solvent. The mole fraction of solute is approximately equal to
A
$$\frac{{{{\text{x}}_1}}}{{{{\text{x}}_2}}}$$
B
$$\frac{{{{\text{x}}_2}}}{{{{\text{x}}_1}}}$$
C
$$1 - \frac{{{{\text{x}}_1}}}{{{{\text{x}}_2}}}$$
D
$$\frac{1}{{{{\text{x}}_2}}}$$
What is the enthalpy change of 8 mole solution if the enthalpy change of 5 mole solute is 10 J/mole, and enthalpy of 2 mole solvent is 15 J/mole?
A
10 J/mole
B
12 J/mole
C
13 J/mole
Two feeds, 10 mole with 5 J/mole and 20 mole with 15 J/mole, product contains two streams, 5 mole with 10 J/mole and P with 25 J/mole, what is the value of P?
A
10 mole
B
12 mole
C
15 mole
Two feeds, 5 mole with 25 J/mole and F with 5 J/mole, product contains two streams, 5 mole with 10 J/mole and 10 mole with 15 J/mole, what is the value of F?
A
10 mole
B
15 mole
C
20 mole
The ratio of existing moles of vapor per mole of vapor free gas to the moles of vapor that would be present per mole of vapor free gas, if the mixture were saturated at the existing temperature & pressure, is termed as the
A
Relative humidity
B
Relative saturation
C
Percentage saturation
D
None of these
In the carbonation of a soft drink, the total quantity of carbon dioxide required is the equivalent of 3 volumes of gas to one volume of water at 0⁰C and atmospheric pressure. Calculate (i) the mass fraction and (ii) the mole fraction of the CO2 in the drink, ignoring all components other than CO2 and water. Basis 1 m3 of water = 1000 kg Volume of carbon dioxide added = 3 m3 From the gas equation, pV = nRT 1 x 3 = n x 0.08206 x 273 n = 0.134 mole. Molecular weight of carbon dioxide = 44 And so weight of carbon dioxide added = 0.134 x 44 = 5.9 kg
A
6.9 × 10-3, 3.41 × 10-3
B
8.9 × 10-3, 2.41 × 10-3
C
5.9 × 10-3, 2.41 × 10-3
D
9.9 × 10-3, 3.41 × 10-3
Vapor pressure of a solution is proportional to (where, S
v
and S
t
are mole fraction of solvent and solute respectively).
A
S<sub>v</sub>
B
$$\frac{1}{{{{\text{S}}_{\text{t}}}}}$$
C
S<sub>t</sub>
D
$$\frac{1}{{{{\text{S}}_{\text{v}}}}}$$
If the partial vapor pressure of the component is 1000pa in the gaseous mixture and the vapor pressure of pure component is 2000pa what is the mole fraction of the solute?
A
2
B
1
C
1.5
D
0.5
Three feeds, 10 mole with H = 5 J/mole, 10 mole with H = 15 J/mole and 5 mole with 20 J/mole, what is the enthalpy of the products?
A
10 J/mole
B
12 J/mole
C
15 J/mole
Three feeds, 10 mole with H = 25 J/mole, 5 mole with H = 10 J/mole and 15 mole with 20 J/mole, what is the enthalpy of the products?
A
10 J/mole
B
12 J/mole
C
20 J/mole