Chemistry · Chemical Equilibrium

A student performs an experiment on the following equilibrium reaction: 2NO2(g) ↔ N2O4(g) ΔH = –57 kJ/mol Two gas syringes containing the same concentrations of brown NO2 gas are placed in different temperature baths. Syringe A is placed in ice water (low temperature) and Syringe B is placed in a hot water bath (high temperature). After equilibrium is reached, Syringe A shows a much paler brown color than Syringe B. Which conclusions are valid? (a) The formation of colorless N2O4 is favored at lower temperatures. (b) Higher temperatures shift equilibrium toward the reactants, favoring NO2. (c) The equilibrium constant (K) increases as the temperature increases for this reaction.