Question

Chemical equation for acid rain and calcium carbonate

Answer 1

Answer:

Explanation:

1. pure water has a pH of 7.0 (neutral); however, natural, unpolluted rainwater actually has a pH of about 5.6 (acidic).[Recall from Experiment 1 that pH is a measure of the hydrogen ion (H+) concentration.] The acidity of rainwater comes from the natural presence of three substances (CO2, NO, and SO2) found in the troposphere (the lowest layer of the atmosphere

n the gas phase sulfur dioxide is oxidized by reaction with the hydroxyl radical via an intermolecular reaction:[5]

SO2 + OH· → HOSO2·

which is followed by:

HOSO2· + O2 → HO2· + SO3

In the presence of water, sulfur trioxide (SO3) is converted rapidly to sulfuric acid:

SO3 (g) + H2O (l) → H2SO4 (aq)

Nitrogen dioxide reacts with OH to form nitric acid

NO2 + OH· → HNO3

Sulfur dioxide dissolves in water and then, like carbon dioxide, hydrolyses in a series of equilibrium reactions:

SO2 (g) + H2O ⇌ SO2·H2O

SO2·H2O ⇌ H+ + HSO3−

HSO3− ⇌ H+ + SO32−

CaCO3(s) + 2 H+(aq) → Ca2+(aq) + CO2(g) + H2O(l)

CaCO3(s) → CaO(s) + CO2(g)

CaCO3(s) + CO2(g) + H2O(l) → Ca(HCO3)2(aq)

CaO + H2O → Ca(OH)2

Ca(OH)2 + CO2 → CaCO3↓ + H2O