what is the molar mass of the unknown gas that diffuses 0.250 times as fast as hydrogen gas under the same circumstances?
time1 = 60 sec = H2
time2 = 240 sec(240*0.25 = 60) = unknown
rate H2 = 1L/60sec
rate unk = 1L/240 sec.
1/60/1/240 = sqrt(M2/2)
Solve for M2.
The time of 60 sec was just made up You may use any convenient time with the corresponding time for the unknown of 4x that.
What hapens you moving from left to right in a periodic table?
To determine the molar mass of the unknown gas, we first need to understand Graham's law of effusion. According to this law, the rate of effusion (or diffusion) of a gas is inversely proportional to the square root of its molar mass.
The equation for Graham's law is as follows:
Rate1 / Rate2 = √(MolarMass2 / MolarMass1)
In this case, we are comparing the rate of effusion of the unknown gas to that of hydrogen gas. Since we are given that the unknown gas diffuses 0.250 times as fast as hydrogen gas, we can write the equation as:
0.250 = √(MolarMassH2 / MolarMassUnknown)
To solve for the molar mass of the unknown gas, we isolate it in the equation:
(MolarMassUnknown) = (MolarMassH2) / (0.250)^2
Now, the molar mass of hydrogen gas (H2) is approximately 2 g/mol. Plugging this value into the equation, we get:
(MolarMassUnknown) = 2 g/mol / (0.250)^2
Calculating the right-hand side of the equation:
(MolarMassUnknown) = 2 g/mol / 0.0625
(MolarMassUnknown) = 32 g/mol
Therefore, the molar mass of the unknown gas is approximately 32 g/mol.