A certain volume of oxgen diffused from a given apparatus in 125 secs.In the same conditions,the same volume of gas N,diffuse in 100 secs.Calculate the relative molecular mass of N.
I got 0.221 is the answer correct.
No. Does a molar mass of 0.221 sound reasonable? Remember H is the lightest element in the periodic table and it is 2 for H2. Maybe you have found a new element? Post your work if you want us to look for the error..
I need an answer
To calculate the relative molecular mass of gas N, we need to use Graham's Law of Diffusion. According to Graham's Law, the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. The equation for Graham's Law is:
r1 / r2 = sqrt(M2 / M1)
Where:
r1 = rate of diffusion of gas 1 (oxygen)
r2 = rate of diffusion of gas 2 (gas N)
M1 = molar mass of gas 1 (oxygen)
M2 = molar mass of gas 2 (gas N)
From the given information, we know that the rate of diffusion of oxygen (r1) is related to the rate of diffusion of gas N (r2) by the equation:
r1 / r2 = 125 / 100
Now, let's calculate the relative molecular mass of gas N using the formula for Graham's Law:
sqrt(M2 / M1) = r1 / r2
Squaring both sides of the equation:
(M2 / M1) = (r1 / r2)²
Now, we substitute the given values into the equation:
(M2 / M1) = (125 / 100)²
Simplifying:
(M2 / M1) = (1.25)²
(M2 / M1) = 1.5625
To get the relative molecular mass of gas N (M2), we need to know the relative molecular mass of oxygen (M1). Since the relative molecular mass of oxygen is known to be 32 g/mol, we can solve for M2:
32 / M1 = 1.5625
Multiplying both sides by M1:
32 = 1.5625M1
Dividing both sides by 1.5625:
M1 = 32 / 1.5625
M1 ≈ 20.48 g/mol
Now, we can substitute the value of M1 into the equation to find M2:
M2 ≈ 1.5625 * 20.48
M2 ≈ 32 g/mol
Therefore, the relative molecular mass of gas N is approximately 32 g/mol.