<span>In the field of science, usually, the product of an experiment is
computed ahead to understand if it reached a specific objective. It would reach
greater than 100% of percent yield if the factors include faster reaction rates;
proper handling of the reactants, no outside contaminants, and the procedure of
the experiment is followed smoothly. It would reach lesser than 100% percent yield
if the experiment is not followed, external factors such as contamination from
the environment (wind, moisture, etc). </span>
Answer:
The required volume of the original sample required is 2 micro liter
Explanation:
assuming the original sample concentration is 1N
after final dilution of 10-2 solution concentration becomes 0.01 N
normality of original sample = 1 N
normality of final solution = 0.01 N
volume of original sample= ?
volume of final solution = 0.2 mL
Considering thef formula below :
N1V1 = N2V2
V1 = (N2V2)/N1
= (0.01*0.2)/1
= 0.002 mL
1 milli liter = 1000 micro liter
0.002 mL = 2 micro liter
The original sample required is 2 micro liter
It’s how many times deez nuz go into that puh
Explanation:
The given data is as follows.
Moles of oxygen gas = 0.150 mol, Moles of nitrogen gas = 0.116 mol
Moles of argon gas = 0.211 mol, Volume of the flask = 0.5 L
Temperature = 298 K
So, total number of moles will be calculated as follows.
= (0.150 + 0.116 + 0.211) mol
= 0.477 mol
Now, using ideal gas equation we will calculate the total pressure of given gas mixture as follows.
PV = nRT
P = 23.34 atm
Mole fraction of gas will be calculated as follows.
Mole fraction =
=
= 0.243
Using Dalton's law,
where, = partial pressure of a gas
= total pressure
= mole fraction of gas
Therefore, putting the values into Dalton's law to calculate the partial pressure of nitrogen gas as follows.
=
= 5.67 atm
Thus, we can conclude that the partial pressure of into the given mixture is 5.67 atm.