Calculate the molar mass of a compound in the Dumas method at `100^(@)C` for which volume of experimental container was 452 ml and the pressure was 745.1 torr. The difference in mass between the empty container and the final measurement was 1.129 gm.
Text Solution
AI Generated Solution
To calculate the molar mass of the compound using the Dumas method, we will follow these steps:
### Step 1: Convert the temperature to Kelvin
The temperature is given as \(100^\circ C\). To convert this to Kelvin, we use the formula:
\[
T(K) = T(°C) + 273
\]
\[
...
Topper's Solved these Questions
MOLE CONCEPT
ALLEN|Exercise Some Solved Examples|9 Videos
MOLE CONCEPT
ALLEN|Exercise Basic Exercise|29 Videos
METALLURGY
ALLEN|Exercise EXERCISE-05 [B]|26 Videos
p-Block Element
ALLEN|Exercise All Questions|20 Videos
Similar Questions
Explore conceptually related problems
A gas is filled in a container at certain temperature and pressure. At the same temperature more gas is filled in the vessel. Calculate the percentage increase in the mass of the gas. If the ratio of initial and final pressure is 1:2.
A gas is filled in a container at certain temperature and pressure. At the same temperature more gas is filled in the vessel. Calculate the percentage increase in the mass of the gas. If the ratio of initial and final pressure is 1:2 .
The percentage change in the pressure of a given mass of a gas filled in a container at constant temperature is 100%. Calculate the percentage change in its volume.
Calculate the vapour pressure of an aqueous solution which contains 5 mass per per cent of urea . The vapour pressure of pure water is 23.5 mm Hg . The molar mass of urea is 60 .
Calculate the molar mass of a substance 1 g of which when dissolved in 100 g of water gave a solution boiling at 100.1^(@)C at a pressure of 1 atm (K_(b) for water = 0.52 K kg mol^(-1))
A gas is filled in a container at 27^@ C . On increasing the temperature to 127^@ C , 1 litre (having (1)/(4) th mass) of the gas escape out of the container. Calculate the volume of the container.
The volume of a given mass of a gas with some pieces of marble in a container at 750 mm Hg pressure is 100 mL. If the pressure is changed to 1000 mm Hg, the new volume is 80 mL. Find the volume occupied by the marble pieces, if the temperature remains constant.
If the density of a gas at the sea level at 0^(@)C is 1.29 kg m^(-3) , what is its molar mass? (Assume that pressure is equal to 1"bar" .)
The vapour pressure of water at 80^(@)C is 355 torr. A 100 ml vessel contains water-saturated oxygen at 80^(@)C , the total gas pressure being 760 torr. The contents of the vessel were pumped into a 50.0 ml vessel at the same temperature. What were the partial pressures of oxygen and of water vapour, what was the total pressure in the final equilibrated state? Neglect the volume of any water which might condense.
The vapour pressure of acetone at 20^(@)C is 185 torr. When 1.2 g of non-volatile substance was dissolved in 100g of acetone at 20^(@)C its vapour pressure was 183 torr. The molar mass (g mol^(-1)) of the substance is:
