need help CHM205 Laboratory Fall 2017 Section:-O Name Dicna Grade 6 g, and is us

Question

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CHM205 Laboratory Fall 2017 Section:-O Name Dicna Grade 6 g, and is used A small gas cylinder containing CH (methane) gas to bubble methane into a container that has been submerged-in-22.0 °C water. The volume of the gas that is inside the eontainer at the end is 0.228 L., and the gas cylinder weighs 246.622 gThe barometric pressure of the room is 1.05 atm. 1. Calculate the mass of CH, that was released into the container 2. Calculate the temperature of the water (and thus the CHa gas) in Kelvins. 3. Find the vapor pressure of water at this temperature (use the chart in the introduction!) 4. Determine the partial pressure being exerted by the CHs in the container, in atm Use the ideal gas law and your calculated data above to calculate the number of moles of CHs that were in the container 5. 6. Use the data from parts 1. and 5, to calculate the experimental molar mass of CH4.

Explanation / Answer

(1)

Mass of gas released into the container = Change in mass of container = 246.776-246.622 = 0.154 g

(2)

Temp of water and gas = 220C = 273+22 = 295 K

(3)

Using the chart we see that vapor pressure of water at this temp = 19.8 torr = 0.026 atm

(4)

Pressure exerted by water + Pressure exerted by methane = 1.05 atm

So,

Pressure exerted by methane = 1.05-0.026 = 1.024 atm

(5)

Using ideal gas equation:

PV = nRT

Putting values:

1.024*0.228 = n*0.0821*295

Solving we get:

n = 0.00964 moles

(6)

Experimental molar mass = Mass/moles = 0.154/0.00964 = 15.975 g

Hope this helps !

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