Which compounds are acting like brønsted-lowry acids in the following acid-base equilibrium?

hco3− + h2o h2co3 and oh−

The compounds HCO₃⁻ and OH⁻ are acting like a Brønsted-Lowry base and the compounds H₂C0₃ H₂0 are acting like a Brønsted-Lowry acid.

Explanation:

According to the Brønsted-Lowry theory an acid is any  species capable of donating a proton (H⁺) and a base is any species capable of accepting a proton (H⁺)

The conjugate base of a Brønsted-Lowry acid is the species that is formed after the acid donates its proton and the conjugate acid of  Brønsted-Lowry base is the species that is formed after the base accepts a proton.

For example:

H₂SO₄ + OH⁻ ⇆ HSO₄⁻ + H₂O

In this equilibrium H₂SO₄ is acting like a Brønsted-Lowry acid and HSO₄⁻ is its conjugate base. Also OH⁻ is acting like a Brønsted-Lowry base and H₂O is its conjugate acid

So, HCO₃⁻ is acting like a Brønsted-Lowry base and H₂C0₃ is its conjugate acid. Also H₂O is acting like a Brønsted-Lowry acid and OH⁻ is its conjugate base.

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.