Gas has a volume of 247.3 ML and is at 100 Celsius and 745 Hg. If the mass of the gas is 0.347 g what is the molar mass of the v
1 answer:
Answer:
The molar mass of the vapor is 43.83 g/mol
Explanation:
Given volume of gas = V = 247.3 mL = 0.2473 L
Temperature = T = 100 = 373 K
Pressure of the gas = P = 745 mmHg (1 atm = 760 mmHg)
Mass of vapor = 0.347 g
Assuming molar mass of gas to be M g/mol
The ideal gas equation is shown below
The molar mass of the vapor comes out to be 43.834 g/mol
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Complete Question
methanol can be synthesized in the gas phase by the reaction of gas phase carbon monoxide with gas phase hydrogen, a 10.0 L reaction flask contains carbon monoxide gas at 0.461 bar and 22.0 degrees Celsius. 200 mL of hydrogen gas at 7.10 bar and 271 K is introduced. Assuming the reaction goes to completion (100% yield)
what are the partial pressures of each gas at the end of the reaction, once the temperature has returned to 22.0 degrees C express final answer in units of bar
Answer:
The partial pressure of methanol is
The partial pressure of carbon monoxide is
The partial pressure at hydrogen is
Explanation:
From the question we are told that
The volume of the flask is
The initial pressure of carbon monoxide gas is
The initial temperature of carbon monoxide gas is
The volume of the hydrogen gas is
The initial pressure of the hydrogen is
The initial temperature of the hydrogen is
The reaction of carbon monoxide and hydrogen is represented as
Generally from the ideal gas equation the initial number of moles of carbon monoxide is
Here R is the gas constant with value
=>
=>
Generally from the ideal gas equation the initial number of moles of Hydrogen is
=>
Generally from the chemical equation of the reaction we see that
2 moles of hydrogen gas reacts with 1 mole of CO
=> 0.064 moles of hydrogen gas will react with x mole of CO
So
=>
Generally from the chemical equation of the reaction we see that
2 moles of hydrogen gas reacts with 1 mole of
=> 0.064 moles of hydrogen gas will react with z mole of
So
=>
From this calculation we see that the limiting reactant is hydrogen
Hence the remaining CO after the reaction is
=>
=>
So at the end of the reaction , the partial pressure for CO is mathematically represented as
=>
=>
Generally the partial pressure of hydrogen is 0 bar because hydrogen was completely consumed given that it was the limiting reactant
Generally the partial pressure of the methanol is mathematically represented as
Here is used because it is given the question that the temperature returned to 22.0 degrees C
So