Consider the combustion of liquid methanol, CH3OH1l2:CH3OH1l2 + 32O21g2¡ CO21g2 + 2 H2O1l2ΔH = -726.5 kJ(a) What is the enthalpy change for the reverse reaction?(b) Balance the forward reaction with whole-number coefficients.What is ΔH for the reaction represented by thisequation? (c) Which is more likely to be thermodynamicallyfavored, the forward reaction or the reverse reaction?(d) If the reaction were written to produce H2O1g2 insteadof H2O1l2, would you expect the magnitude of ΔH to increase,decrease, or stay the same? Explain.

Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic     (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =   kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?  g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =  kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K   kJ HopHelpCh5N1

(b)  Calculate the enthalpy change for the reaction C(graphite) + 2 H2(g) → CH4(g) with the help of the enthalpy changes of the following reactions: C(graphite) + O2(g) → CO2(g) ∆H= -393.5 kJmol−1 H2(g) +1/2O2(g) → H2O(l) ∆H = -285.8 kJmol−1 CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H = -890.4 kJmol−1 The temperature is 25 ◦C in all instances.

iv to vi please