Gaseous carbon monoxide and hydrogen gas can be used to prepare methanol (CH₃OH). Under equilibrium conditions at 427°C, the partial pressures of the components are as follows.
P_CO = 1.44 atm $P _ { \mathrm { H } _ { 2 } }$
= 4.25 atm $P _ { \mathrm { CH } _ { 3 } \mathrm { OH } }$
= 2.30 atm
What is the value of the equilibrium constant for the reaction in which one mole of methanol is produced?

Question

Gaseous carbon monoxide and hydrogen gas can be used to prepare methanol (CH₃OH). Under equilibrium conditions at 427°C, the partial pressures of the components are as follows.
P_CO = 1.44 atm

P _ { \mathrm { H } _ { 2 } }

= 4.25 atm

P _ { \mathrm { CH } _ { 3 } \mathrm { OH } }

= 2.30 atm
What is the value of the equilibrium constant for the reaction in which one mole of methanol is produced?

Quizplus · Accepted Answer

The Answer of Gaseous carbon monoxide and hydrogen gas can be used to prepare methanol (CH₃OH). Under equilibrium conditions at 427°C, the partial pressures of the components are as follows. P_CO = 1.44 atm $P _ { \mathrm { H } _ { 2 } }$ = 4.25 atm $P _ { \mathrm { CH } _ { 3 } \mathrm { OH } }$ = 2.30 atm What is the value of the equilibrium constant for the reaction in which one mole of methanol is produced?

Gaseous Carbon Monoxide and Hydrogen Gas Can Be Used to Prepare