Please answer I have a finals and I need help with a question similar!!! 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 °C. 345 mL of hydrogen gas at 7.12 bar and 271 K is introduced. Assume 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 to22.0 °C?. units in bar please

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

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

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