For a gaseous reaction, standard conditions are 298 K298 K and a partial pressure of 1 bar1 bar for all species. For the reaction C2H6(g)+H2(g)↽−−⇀2CH4(g) C2H6(g)+H2(g)↽−−⇀2CH4(g) the standard change in Gibbs free energy is ΔG∘=−32.8 kJ/mol.ΔG°=−32.8 kJ/mol. What is ΔGΔG for this reaction at 298 K298 K when the partial pressures are PC2H6=0.200 bar, PC2H6=0.200 bar, PH2=0.450 bar, PH2=0.450 bar, and PCH4=0.600 bar?

Hi + naoh -> h2o + nal

Reaction involved in present system is :   c12h22o11 + h2o → 2 c6h12o6the reaction system is obeying following rate law:   rate = k[c12h22o11]thus, it is a first order reaction.now, for 1st order reactionrate constant (k) =  given: initial conc. = 3.0 g, final conc. = 2.7 g, t = 2.5 h∴rate constant (k) =  ∴ k = 0.04215 h-1now, for 1st order reaction, half life = 0.693/k = 0.693/0.04215 = 16.4 hthus correct answer is option b