What happens to the value of the equilibrium constant for a reaction if the reaction equation is reversed? Multiplied by a constant?

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8 (g) + 5 O2 (g) <---> 3CO2 (g) + 4 H2O (l).    Delta H = -2220 kJ     The reaction will shift to the right in the direction of products.     No effect will be observed.     The equilibrium constant will increase.     The equilibrium constant will decrease.     The reaction will shift to the left in the direction of reactants.

What does Le Chatelier's principle state? • A reaction can proceed both forward and backward in a state of equilibrium • reactions only occur when particles collide with enough energy and in the right orientation to react • some reactions can only proceed in one direction, not in both directions •

Explain a condition that could be changed in a system that would increase the amounts of products at equilibrium and explain why this happens.

The equilibrium system between nitrogen gas, oxygen gas, and nitrogen dioxide gas is given.   N2(g)+2O2(g)↽−−⇀ 2NO2(g)N2⁡(g)+2⁢O2⁡(g)⁢↽−−⇀ 2⁢NO2⁢(g)   Write the balanced chemical equation for the reverse reaction. Include physical states for all species. chemical equation:

If the equilibrium constant for an equilibrium system has decreased because of a "stress", how have the concentrations changed? O [reactants] and [products] decreases [reactants] decreases and [products] increases O [reactants] increases and [products] decreases [reactants] and [products] increases

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 200. mL flask with 4.3 atm of carbon monoxide gas and 4.1 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.5 atm of carbon monoxide gas, 1.3 atm of water vapor and 2.8 atm of carbon dioxide. The engineer then adds another 1.1 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 O

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 5.0 L flask with 4.3 atm of sulfur dioxide gas and 3.9 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 3.9 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K, = 0

If the equilibrium constant of a given reaction is 6.96, what is the equilibrium constant of its reverse reaction?

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 500. mL flask with 1.2 atm of sulfur dioxide gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.60 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K, -0 x10 5