A mixture of two gases has a total pressure of 5.7 atm . If one gas has a partial pressure of 4.1 atm , what if the partial pres
2 answers:
Answer:
1.6 atm
Explanation:
We are given that total pressure of mixture of two gases=5.7 atm
Partial pressure of one gas=4.1 atm
We have to find the partial pressure of other branch.
We know that Dalton;s law of partial pressure
It states that pressure exerted by mixture of gases is equal to sum of partial pressure exerted by gases in mixture.
Let x bet the pressure exert by other gas
Apply this law
Total pressure=4.1+x
Hence, the partial pressure of other gas=1.6 atm.
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Answer:
A breakdown of the breaking buffer was first listed with its respective component and their corresponding value; then a table was made for the stock concentrations in which the volume that is being added was determined by using the formula . It was the addition of these volumes altogether that make up the 0.25 L (i.e 250 mL) with water
Explanation:
Given data includes:
Tris= 10mM
pH = 8.0
NaCl = 150 mM
Imidazole = 300 mM
In order to make 0.25 L solution buffer ; i.e (250 mL); we have the following component.
Stock Concentration Volume to be Final Concentration
added
1 M Tris 2.5 mL 10 mM
5 M NaCl 7.5 mL 150 mM
1 M Imidazole 75 mL 300 mM
. is the formula that is used to determine the corresponding volume that is added for each stock concentration
The stock concentration of Tris ( 1 M ) is as follows:
.
The stock concentration of NaCl (5 M ) is as follows:
.
The stock concentration of Imidazole (1 M ) is as follows:
.
Hence, it is the addition of all the volumes altogether that make up 0.25L (i.e 250 mL) with water.