Le Chatelier's principle

For the reaction below, (metane gas reacting with dihydrogen sulfide) which change would cause the equilibrium to shift to the right?

CH_4(g) + 2H₂S_(g) ↔ CS_2(g) + 4H_2(g)

• Decrease the concentration of dihydrogen sulfide.

• Increase the pressure on the system.

• Increase the temperature of the system.

• Increase the concentration of carbon disulfide.

• Decrease the concentration of methane.

Tags

NGSS.HS-PS1-6

Equiliblrium is a state of dynamic molecular behavior, meaning that

• the reaction eventually comes to a stop.

• reactants continually turn into products at a progressively slower rate.

• products continually turn into reactants at a progressively faster rate.

• reactants turn into products and products turn into reactants at different rates.

• reactants turn into products and products turn into reactants at equal rates.

Which of the below are ways that allow you to recognize equilibrium?

• constant temperature

• constant color

• constant pressure

• All the options are correct.

Consider the following reaction:

Fe ⁺³ + SCN ↔ FeSCN ²⁺

(Light Yellow) (Deep Red)

Adding Fe(NO₃)₃ produced the following change in the equilibrium:

• The color in the test tube became a deeper red color because the equilibrium shifted to make more reactants.

• The color in the test tube became a deeper red color because the equilibrium shifted to make more products.

• The color in the test tube became a lighter color because the equilibrium shifted to make more reactants.

• The color in the test tube became a lighter color because the equilibrium shifted to make more products.

Tags

NGSS.HS-PS1-5

Consider the following reaction:

Fe ⁺³ + SCN ↔ FeSCN ²⁺

(Light Yellow) (Deep Red)

Adding AgNO₃ to the test tube removed SCN ^- from the reaction, causing the reaction to

• produce more reactants and decrease the amount of products.

• decrease the amount of products causing a deeper color.

• produce a deeper red color because the production of more reactants.

Tags

NGSS.HS-PS1-5

Consider the following reaction:

Fe ⁺³ + SCN ↔ FeSCN ²⁺

(Light Yellow) (Deep Red)

The reaction you studied is became a deeper red color when placed in an ice bath. This means that the reaction is

• exothermic.

• endothermic.

• There is not enough information given to answer the qusestion.

• None of the above are correct.

Tags

NGSS.HS-PS1-5

In the reaction N₂O_{4 (g)} ↔ 2 NO_{2 (g)}, an increase in pressure (by reducing the volume) would make the reaction

• form more products.

• form more reactants.

• Increasing the reaction would have no effect on the equilibrium.

• There is not enough information given to answer the question.

In the reaction, CO _(g) + NO_{2 (g)} ↔ CO_{2 (g)} + NO _(g), which of the following changes would result in the formation of more products at equilibrium?

• increasing the pressure

• removing CO (g) from the reaction

• adding NO₂ (g) to the reaction

• adding CO₂ to the reaction.

• None of the options would result in more products.