Answer:
They meet at the distance of 32.5 cm
Explanation:
The rate of diffusion is inversely proportional to the molar mass of gases.
If diffusion is represented as d and mass of gases as M. Then , rate is given as:

For , two gases

First , Calculate the ,molar mass of each gas :
CH4 = 1 (mass of C) + 4(mass of H)
= 1(12)+4(1)
= 12 + 4 = 16 gram
M1 = 16 gram
C4H8 = 4(mass of C) + 8(Mass of H)
= 4(12) + 8(1)
= 48 + 8
M2 = 56 grams
d1 is diffusion of CH4
d2 = diffusion of C4H8

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This means CH4 diffuse 1.87 times faster than C4H8
Now, the mathematical part
If velocity of C4H8 = 1 cm/sec , then velocity of CH4 = 1.87 cm/sec
v1 = 1.87 cm/sec
v2 = 1 cm/sec
Let both meet at time "t". If distance travelled by CH4(s1) = x , then remaining(s2) distance (50-x) is travelled by C4H8
(see the attached image)

since both meet at same time so t = constant.


on solving for x we get,
x = 17.42 cm
from the other side the distance is (50 - x)
= 50 - 17.42 = 32.5 cm
Answer:
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Answer:
Argument: It is not Safe
Further support to the argument is given below.
Explanation:
Solution:
Argument: It is not Safe
First of all, we all know the ideal gas law:
PV = nRT
And the Boyle's Law states that , if the pressure is increased then, volume will decrease. and if the volume is increased then pressure will decrease.
V is inversely proportional to Pressure of the gas.
So, in this case, Let's suppose we have toxic solution of methyl alcohol in the bottle which is tightly closed. It means pressure in the bottle is high, hence the volume is less.
If in this scenario someone, leave the bottle open in the laboratory and as it is given that the level of solution will drastically decrease. It means it is volatile in nature and is converted into gaseous form and we know now that the open bottle has now less pressure. Hence the volume of the gas will be higher and now it can spread to every corner of the laboratory. And it is very dangerous.