A sample of pure NH4HS is placed in a sealed 2.0-L container and heated to 550 K at which the equilibrium constant is 3.5 x 10-3. Once the reaction reaches equilibrium, what mass of NH3 is present in the container

The mass of in the container is 2.074 gram

Explanation:

Given:

Volume of     lit

Equilibrium constant

The reaction in which is produced

  ⇄

Here equal moles of and is formed.

From the formula of equilibrium constant,

      M

Above value shows,

So in 2 L no. moles of = moles.

So mass of 0.122 mole of is = g

Therefore, the mass of in the container is 2.074 gram

the only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation:

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation: