Under the same temp.and pressure ,nitrogen gas diffuses 8 times as fast as gas y .calculate the relative molecular mass of gas y.
I can't see the solution to my question
To calculate the relative molecular mass of gas Y, we can 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.
Given that nitrogen gas (N2) diffuses 8 times faster than gas Y, we can write the following equation:
rate of diffusion of N2 / rate of diffusion of Y = √(molar mass of Y / molar mass of N2)
Let's assume the molar mass of nitrogen gas (N2) is M_N2, and the molar mass of gas Y is M_Y.
Given that nitrogen gas diffuses 8 times faster than gas Y, we can substitute the values into the equation:
8 = √(M_Y / M_N2)
To solve for the relative molecular mass of gas Y (M_Y), we need to square both sides of the equation:
8^2 = (√(M_Y / M_N2))^2
64 = M_Y / M_N2
Now, we rearrange the equation to find the relative molecular mass of gas Y:
M_Y = 64 * M_N2
Therefore, the relative molecular mass of gas Y is 64 times the molar mass of nitrogen gas (N2).