In a closed 1.00 L flask, 4.30 atm of CO reacts with 2.50 atm of O2...

In a closed 1.00 L flask, 4.30 atm of CO reacts with 2.50 atm of O2 according to the equation below. Assuming that the temperature remains constant, what is the final pressure in the flask?

Expert Solution

2CO + O2------> 2CO2

2 moles 1 mole

4.3 atm 2.5 atm 0 initial

-4.3 atm - 2.15 atm 4.3atm change

0 0.35atm 4.3 atm at euilibrium

from the balanced equation

2 moles of CO react with 1 moles of O2

4.3 atm of CO react with = 4.3/2 = 2.15 atm of O2

Here limiting reagent is CO

2 moles of CO react with O2 to form 2 moles of CO2

4.3 atm of Co react with O2 to form 4.3 atm of CO2

remaing pressure of O2 = 2.5-2.15 = 0.35 atm

total pressure of the flask = PO2+ PCO2

= 0.35 + 4.3= 4.65 atm

queen_honey_blossom answered 2 years ago

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