A large container (20.0 Liters) contains a few mL of liquid water.It also contains 0.0414 moles of Argon gas and 0.0384 moles of CO2 gas.The temperature is 35. °C.(a) What is the partial pressure of water in this flask?(b) How many moles of water are in this flask?(Take the volume of gas to be 20.0 L.)(c) What are the partial pressures of the CO2 and the Ar?(d) What is the total pressure? Vapor Pressure ofwater in torTemperature in °C(P1,0)1916.52017.52118.72219.82321.12422.42523.82625.22726.72828.42930.03031.53236.03542.04055.55092.360149.3

Dalton's law of partial pressure:- This law is made to find the partial pressure of gases from the…

Answered: A large container (20.0 Liters)…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

A large container (20.0 Liters) contains a few mL of liquid water.
It also contains 0.0414 moles of Argon gas and 0.0384 moles of CO2 gas.
The temperature is 35. °C.
(a) What is the partial pressure of water in this flask?
(b) How many moles of water are in this flask?
(Take the volume of gas to be 20.0 L.)
(c) What are the partial pressures of the CO2 and the Ar?
(d) What is the total pressure?

Vapor Pressure of
water in tor
Temperature in °C
(P1,0)
19
16.5
20
17.5
21
18.7
22
19.8
23
21.1
24
22.4
25
23.8
26
25.2
27
26.7
28
28.4
29
30.0
30
31.5
32
36.0
35
42.0
40
55.5
50
92.3
60
149.3

Expert Solution

Step 1

Dalton's law of partial pressure:- This law is made to find the partial pressure of gases from the mixture of gases present in a system, by adding the partial pressure of the component of gases in the mixture of gases present.

Moreover, it can also be find by the product of mole fraction of gas and the total pressure in the mixture of gases present in the system.

$\begin{array}{rcl} P_{g} & = & x_{g} . P_{T o t a l} \\ a n d, P_{Total} & = & \frac{P_{g}}{x_{g}} \\ w h e r e, \\ P_{g} & = & p a r t i a l p r e s s u r e o f g a s \\ x_{g} & = & m o l e f r a c t i o n o f g a s \\ P_{T o t a l} & = & t o t a l p r e s s u r e o f t h e s y s t e m \\ A n d, \\ x_{g} & = & \frac{n u m b e r o f m o l e s o f g a s}{t o t a l n u m b e r o f m o l e s o f m i x t u r e o f g a s e s} \end{array}$

Ideal gas equation (used to calculate the required terms) is as follows:-

$\begin{array}{rcl} P V & = & n R T \\ w h e r e, \\ P & = & p r e s s u r e o f t h e i d e a l g a s \\ V & = & v o l u m e o f t h e i d e a l g a s \\ n & = & n u m b e r o f m o l e s o f i d e a l g a s \\ R & = & U n i v e r s a l g a s c o n s \tan t = 62.36 L . t o r r . K^{- 1} . m o l^{- 1} \\ T & = & t e m p e r a t u r e o f i d e a l g a s [i n k e l v i n (K)] \end{array}$

Temperature=35 $° C$ =273.15+35=308.15K

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