please show all work. all answers shown are incorrect. My molar ratio is 1.200

Methanol (C) is formed from carbon monoxide (A) and hydrogen (B) in the gas-phase reaction CO+2H CH3OH The mole fractions of the reactive species at equilibrium satisfy the relation Ye P/2 Keg (T) where P is the total pressure (atm), Keq the reaction equilibrium constant (atm 2), and T the temperature (K). The equilibrium constant Keq equals 10.5 at 373 K, and 2.316 x 10-4 at 573 K. A semilog plot of Keq (logarithmic scale) versus 1/T (rectangular scale) is approximately linear between T = 300 K and T = 600 K. a. What is the value of log10(Keq x (1 atm)2) at T=422 K? i 0,317 b. Suppose you begin with a molar ratio of CO/H = 1.200 and no methanol. If the reaction proceeds to equilibrium at 422 K and 2 atm, calculate the molar composition of the product and the fractional conversion of CO. Yco: 0.468 YH: 0.425 &200 b. Suppose you begin with a molar ratio of CO/H = 1.200 and no methanol. If the reaction proceeds to equilibrium at 422 K and 2 atm, calculate the molar composition of the product and the fractional conversion of CO. i Yco: 0.468 0.425 0.1066 0.1855 Y CHOH Fractional Conversion: M. c. Repeat the calculation for a molar ratio of CO/H = 1.450. i 6.54 Yco: ,: 0.367 YCH, OH i 0.042 Fractional Conversion: i 14.52