We can't use the nitrogen present in the atmosphere although 80% of the atmosphere consists of nitrogen only.We get this from the plants called as leguminous plants which can convert or fix atmospheric nitrogen into usable ones..
Answer:
to show that atoms are conserved in chemical reactions
Explanation:
The patient needs 1000 ml of 5% (w/v) glucose solution
i.e 1000 ml x 5 g/ 100 ml
where the stock solution is 55% (w/v) = 55 g / 100 ml
So, 1000 ml x 5 g / 100 ml = V (ml) x 55 g / 100 ml
V = 1000 x (5 / 100) / (55 / 100) = 5000 / 55 = 90.9 ml
∴ the patient needs 90.9 ml of 55% (w/v) glucose solution
Answer:
2,4-di Ethyl-2-methylpentane
C10H22
3,4 dimethyl heptane
C9H20
Explanation:
Answer:
The volume of the vessel is 250 L
Partial pressure of hydrogen = 189 torr
Explanation:
Using Boyle's law
![{P_1}\times {V_1}={P_2}\times {V_2}](https://tex.z-dn.net/?f=%7BP_1%7D%5Ctimes%20%7BV_1%7D%3D%7BP_2%7D%5Ctimes%20%7BV_2%7D)
Given ,
V₁ = 20.0 L
V₂ = ?
P₁ = 25 atm
P₂ = 2 atm
Using above equation as:
![{P_1}\times {V_1}={P_2}\times {V_2}](https://tex.z-dn.net/?f=%7BP_1%7D%5Ctimes%20%7BV_1%7D%3D%7BP_2%7D%5Ctimes%20%7BV_2%7D)
![{25}\times {20.0}={2}\times {V_2}](https://tex.z-dn.net/?f=%7B25%7D%5Ctimes%20%7B20.0%7D%3D%7B2%7D%5Ctimes%20%7BV_2%7D)
![{V_2}=\frac {{25}\times {20.0}}{2}\ L](https://tex.z-dn.net/?f=%7BV_2%7D%3D%5Cfrac%20%7B%7B25%7D%5Ctimes%20%7B20.0%7D%7D%7B2%7D%5C%20L)
![{V_2}=250\ L](https://tex.z-dn.net/?f=%7BV_2%7D%3D250%5C%20L)
<u>The volume of the vessel is 250 L.</u>
According to Dalton's law of partial pressure:-
![P_{H_2}=Mole\ fraction\times Total\ Pressure](https://tex.z-dn.net/?f=P_%7BH_2%7D%3DMole%5C%20fraction%5Ctimes%20Total%5C%20Pressure)
So, according to definition of mole fraction:
![Mole\ fraction\ of\ H_2=\frac {n_{H_2}}{n_{H_2}+n_{He}}](https://tex.z-dn.net/?f=Mole%5C%20fraction%5C%20of%5C%20H_2%3D%5Cfrac%20%7Bn_%7BH_2%7D%7D%7Bn_%7BH_2%7D%2Bn_%7BHe%7D%7D)
Also,
Mole fraction of H₂ = 1 - Mole fraction of He = 1 - 0.75 = 0.25
So,
Total pressure = 756 torr
Thus,
![P_{H_2}=0.25\times 756\ torr](https://tex.z-dn.net/?f=P_%7BH_2%7D%3D0.25%5Ctimes%20756%5C%20torr)
<u>Partial pressure of hydrogen = 189 torr.</u>