it was found that in an experiment tthat a gas c diffuses 8.76¡Á10^-1 times faster than nitrogen gas calculate the molecular mass of gas c (n=14)
Read the post and clean up the gibberish. And N will be 28 and not 14.
No idea
To calculate the molecular mass of "gas c," we need to use Graham's law of diffusion, which states that the rate of diffusion of a gas is inversely proportional to the square root of its molecular mass.
Let's denote the rate of diffusion for "gas c" as R(c), and for nitrogen gas as R(N). According to the information given, gas c diffuses 8.76 × 10^-1 times faster than nitrogen gas. Therefore, we can write the following equation:
R(c) = 8.76 × 10^-1 × R(N)
Now, let's substitute the formula for the rate of diffusion:
R(c) = (1/√(molar mass of c)) × (1/√(molar mass of N))
R(N) = (1/√(molar mass of N)) × (1/√(molar mass of N))
Since we want to find the molecular mass of gas c, we can represent it as molar mass of c.
Now, let's substitute R(c) and R(N) into the equation:
(1/√(molar mass of c)) × (1/√(molar mass of N)) = 8.76 × 10^-1 × (1/√(molar mass of N))
Simplifying the equation:
√(molar mass of c) = 1 / (8.76 × 10^-1) = 1.14
Next, square both sides of the equation:
molar mass of c = (1.14)^2 = 1.2996
Since the atomic mass unit (amu) is the appropriate unit for molecular mass, we'll round our answer to the nearest whole number. Therefore, the molecular mass of gas c is approximately 1 amu.