Question

A mass of 9.98 g carbon monoxide is reacted with 5.68 g hydrogen to form methanol. CO) + 2 H2CH3OH) The reaction is performed in a 5.00 L flask at 85.0 °C and proceeds to completion. What is the partial pressure (in mmHg) of each of the three species following completion of the reaction? What is the total pressure in the flask? со H2 CH3OH Total mmHg x mmHg * mmHg * mmHg x

Answer 1

1 mol CO 0.356 mol CO No of moles of CO 9.98 g x 28.01 g 1mol H 2.016 g No of moles of H = 2.82 mol H2 5.68 g x Equation: CO 2H- >CH3OH 1 mol CH OH 0.356 mol CO x. No of moles of CH2OH produced from CO 1 mol CO 0.356 mol CHOH 1 mol CHOH 2 mol H2 No of moles of CH2OH produced from H 2.82 mol H x- - 1.41 mol CHOH Since CO imits the production of CH2OH, CO acts as the limiting reactant and H, is the reactant present in excess CO completely reacts out 2 mol H2 0.712 mol H No of moles of H reacted - 0.356 mol CO x- 1mol CO No of moles of H, remains 2.82 mol -0.712 mol 2.108 mol No of moles of CO remains 0 Pressure of CO, Po = 0 mmHg No of moles of H, remains= 2.108 mol nRT Pressure of H2 , V LmmHg (85° C+273)K (2.108 mol) 62.4 Kmol 5.00 L =9418 mmHg No of moles of CHOH produced= 0.356 mol nRT Pressure of CH3OH,PH0H LmmHg 85 C+273)K (0.356 mol) 62.4 Kmol 5.00 L 1590 mmHg Total pressure, ptal = Pco+ Рен,дн =0 mmHg 9418 mmHg 1590 mmHg 11008 mmHg