Study the following equation. Fe(s) + 2 HCl(aq) → H2(g) + FeCl2(aq)

What happens to the iron metal when it is reacted in a closed container to produce hydrogen gas in this manner?

Select all that apply.

The rate of the reverse reaction increases as hydrogen gas accumulates. (correct)

The rate of the forward reaction is at its maximum when the reaction first starts.

The rate of the reverse reaction decreases as pressure from the hydrogen gas accumulates.

the answer is a. co2, this would be colder than the : )

explanation:

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24

i think its 5049.

i hope this !

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.