Question

Consider the following reaction: CO(g) + 2 H2(g) → CH2OH (9) AH = -90.7 kJ Calculate the amount of heat transferred when 107.3 g of CH2OH is synthesized by the above reaction at constant pressure. Select one: oa. -90.7 kJ ob. 9.732 x 102 kJ O C. 3.037 x 102 kJ O d. -3.037 x 102 kJ o e. 9.732 x 10 kJ Consider the following reaction: CO(g) + 2 H2 (g) → CH3OH (9) AH = -90.7 kJ For a given sample of Co, the enthalpy change upon reaction is -32.7 kJ. How many grams of hydrogen gas are consumed in the process? Select one: a. 727 g b.7.27 x 10-29 c. 1.45 x 10g d.0.727 g

Answer 1

(1) The Chemical Reaction is given as: Cog, + 2H2 CH₂ OH AH-90.7 kJ => from the stochiometry of above cl reaction we have a mole of Hy to 1 mole of Co reacts with give 1 mole of cl₂oH. = 3.2004 - 9o.7kJ int of heat transferred When 1 mole je 329 1 mol of CH₃OH is Synthesized - 90.7 kJ Amount of Heat transferred When 1g of CH₂ OH is synthesized = -90.7 KI 32.04 i Amount of Heat transferred when 107.3 g of CH₂OH in Synthesized is given as: - =) - 90.7 x 107.3 1-3:037 10 KJ (1) from the Chemical reaction we have. =) -90.7kJ energy is Buy Produced when 28g/mol of Co reacts with 4.032g of hydrogen. 1k5 of energy is produced by = 28 g - 32.7 kJ of energy is produced by = 28 x-32.7 => 1 10.09ug of co Thus 20 g of co require hyetragen - 4.032g Ig of co require hydrogen = 4:0329 : 10.09ug will require hydrogen a 4.032 x 10.094 - 90.7 28