[
1
2
.
1
6
]
A solution is
4
0
.
0
%
by mass benzene
(
CoH
6
)
in carbon tetrachloride
(
CCI
4
)
at
2
0
\
deg C
.
Thevapor pressure of pure benzene and pure carbon tetrachloride at this temperature is
7
4
.
6
1
mmHg and
9
1
.
3
2
mmHg
,
respectively. Calculate the vapor pressure of the solution at
2
0
\
deg C:

Question

[
1
2
.
1
6
]
 ﻿A solution is 
4
0
.
0
%
 ﻿by mass benzene 
(
CoH
6
)
 ﻿in carbon tetrachloride 
(
CCI
4
)
 ﻿at 
2
0
\
deg C
.
 ﻿Thevapor pressure of pure benzene and pure carbon tetrachloride at this temperature is 
7
4
.
6
1
mmHg and 
9
1
.
3
2
 ﻿mmHg
,
 ﻿respectively. Calculate the vapor pressure of the solution at
2
0
\
deg C:

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Calculate the mole fraction of benzene**: The mole fraction of benzene in the solution can be calculated using the percentage by mass and the molar masses of benzene ($C_6H_6$) and carbon tetrachloride ($CCl_4$). ‖ ‖ 2 ⋮ **Apply Raoult's Law**: Raoult's Law states that the vapor pressure of a solution is equal to the mole fraction of the solvent times the vapor pressure of the pure solvent. Here, we will calculate the partial vapor pressures of benzene and carbon tetrachloride in the solution. ‖ ‖ 3 ⋮ **Calculate the total vapor pressure**: The total vapor pressure of the solution is the sum of the partial vapor pressures of benzene and carbon tetrachloride. ‖ ∻Answer∻ ⚹ [Insert final answer here] ⚹ ∻Key Concept∻ ⚹ Raoult's Law and vapor pressure of solutions ⚹ ∻Explanation∻ ⚹ Raoult's Law is used to calculate the vapor pressure of a solution based on the mole fraction of the components and their respective vapor pressures as pure substances. ⚹◊What is the formula for calculating the vapor pressure of a solution according to Raoult's Law?⍭ Generate me a similar question◊

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