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128 ml is the voume of the balloon if the temperature of the gas increases to 320.0k.
Explanation:
given that:
T1 (initial temperature) = 300K
V1 ( initial volume) = 120ml
T2 (final temperature) = 320 K
V2 (final volume) = ?
Pressure remained constant throughout the process.
From the equation
=
Since pressure is constant the equation will be:
=
V2 =
Putting the values in the above formula:
V2 =
= 128 ml
128 ml is the volume of the gas if temperature increases from 3OO K to 320k
Answer:
126.73 mL
Explanation:
The total pressure of the gas mixture is the sum of the vapor pressure of its constituents. So, the vapor pressure of N₂O(p) can be calculated:
750 = 18.85 + p
p = 750 - 18.85
p = 731.15 torr
It means that for 731.15 torr, N₂O occupied 130 mL. For the general gas equation, we know that
Where <em>p</em> is the pressure, <em>V</em> is the volume, <em>T</em> is the temperature, 1 is the initial state, and 2 the final state. For the same temperatue (21ºC), the equation results on Boyle's law:
p1V1 = p2V2, so:
731.15x130 = 750xV2
750V2 = 95049.5
V2 = 126.73 mL
Answer:
Composition of the mixture:
%
%
Composition of the vapor mixture:
%
%
Explanation:
If the ideal solution model is assumed, and the vapor phase is modeled as an ideal gas, the vapor pressure of a binary mixture with and
molar fractions can be calculated as:
Where and
are the vapor pressures of the pure compounds. A substance boils when its vapor pressure is equal to the pressure under it is; so it boils when
. When the pressure is 0.60 atm, the vapor pressure has to be the same if the mixture is boiling, so:
With the same assumptions, the vapor mixture may obey to the equation:
, where P is the total pressure and y is the fraction in the vapor phase, so:
%
The fractions of B can be calculated according to the fact that the sum of the molar fractions is equal to 1.