Henri Le Chatelier's discovery that acetylene and oxygen produced a type of flame far hotter than any flame that was known during his time ultimately led to the invention of what industrial technique? coking in metallurgy false recycling of steel false oxy-acetylene welding true smelting of titanium false Single You can determine how a reversible reaction will progress if you know its Q_c false K_c false Q_c and K_c true rate law false Single Which of the following expressions describes the Q_c of a reversible reaction at equilibrium? Q_c = -∞ false Q_c < 0 false Q_c = 0 false Q_c = K_c true Single What type of reaction is represented by a chemical equation that includes heat as part of the “products”? endothermic reaction false exothermic reaction true may be endothermic or exothermic false both endothermic and exothermic false Single According to the Le Chatelier’s principle, what type of change will a system in equilibrium experience when an external stress acts upon it? It will revert to its initial state false It will adjust to a new state of equilibrium true It will reach a state that would require more energy to change false It will resist changes to its state false Single How will an exothermic reversible reaction in equilibrium offset any additional heat it receives? It will produce more reactants true It will produce more products false It will release more heat false It will stop proceeding spontaneously false Single What is the difference between Q_c and K_c? Q_c represents non-equilibrium concentrations true K_c represents non-equilibrium concentrations false Q_c is always lower than K_c false Q_c is always higher than K_c false Single A reaction took place in a vessel where liquid reactants X and Y produced a solid product W. How will expanding the volume of the vessel affect the reaction? More X and Y will be produced false More W will be produced false The amounts of X, Y, and W will all increase false There will be no change in the amounts of X, Y, and W true Single What will happen to the direction of a reversible reaction when its Qc becomes less than its Kc? It will favor product formation true It will favor reactant formation false It will favor simultaneous product and reactant formation false The progression of a reaction becomes irreversible false Single How can you make a reversible reaction in equilibrium yield more reactants? remove products from the reaction vessel false remove reactants from the reaction vessel true increase the pressure acting on the system false decrease the temperature of the system false Single