Liquid methanol (CH3OH) can be used as an alternative fuel inpickup and SUV engi

Question

Liquid methanol (CH3OH) can be used as an alternative fuel inpickup and SUV engines. An industrial method for preparing it usesthe catalytic hydrogenation of carbon monoxide: CO(g) + 2H2(g) ----->CH3OH(l) How much heat (in kJ) is released when 15.0 L of CO at 85degrees celsius and 112 kPa reacts with 18.5 L of H2 at 75 degreesC and 744 torr? CO(g) + 2H2(g) ----->CH3OH(l) How much heat (in kJ) is released when 15.0 L of CO at 85degrees celsius and 112 kPa reacts with 18.5 L of H2 at 75 degreesC and 744 torr?

Explanation / Answer

We Know that :      The given Reaction is :           CO(g) +2H2(g) ----->CH3OH(l)         H(rxn.) = H (products) - H(reactants)        According to idealgas equation:           PV = nRT           n (CO) = 1.14 atm x 15.0 L / 0.0821 atm-L / mol-Kx 358 K                         = 0.5817 moles            n (H2) =   1.011 atm x 18.5 L/   0.0821 atm-L / mol-K x 348K                            = 0.654 moles           From the above balanced equation it is clear that 1 moleof CO reacts with 2 molesH2                  So forthe given data number of moles of H2   acts as limiting reagent.              for 2 moles of hydrogen 1 mole of methanol is formed in thebalanced equation                    0.654 moles of hydrogen    0.327 moles of methanolis formed           H (rxn.) = H (products) - H(reactants)                            = 0.5817 moles x -238.6 KJ / mol - [ 0.327 moles x -110.5 KJ / mol + 0.654 moles x 0 ]                             = -102.66 KJ

Related Questions

Navigate

• Browse (All)
• Browse L
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.