sulfur
oxides, when dissolved in rainwater, formed sulfuric acid and hence "acid rain." How many metric
tonnes of Indiana coal, which averages 3.5% sulfur
by weight, would yield the H2S04 required to produce a 0.9-in. rainfall of pH 3.90 precipitation over
a 104
 square mile area?

I need help figurng out this challenging problem.

A particular coal contains 2.55% sulfur by mass. When thecoal isburned, it produces SO₂ emissions whichcombine withrainwater to produce sulfuric acid.

PART A

Use the formula of sulfuric acid to calculate the mass percent of Sin sulfuric acid.

? %S

PART B

Determine how much sulfuric acid (in metric tons) is produced bythecombustion of 1.2 metric ton of this coal. (A metricton is 1000kg.)
Express your answer using two significant figures.

m= ? metric ton H₂SO₄

Given information: average sample was 109.16 british grains ofsulfuric anhydride per british gallon of rain water. Sulfuricanahydride is SO3; dissolved in water, each mole of SO3 becomes amole of sulfurous acid, H2SO4

Question: what volume of a 5.00 mM potassium hydroxide solutionwould be required to neutalize 1.00 British gallon of glasglow rainwater?

a) The partial pressure of CO2 in air saturated with water vapor at 25C and 1atm is 3.04E-4 atm. Henry's constant for CO2 is 2.3E-2, and for carbonic acid PKa1=6.37. Assuming that all the dissolved CO2 can be thought of as H2CO3, verify the calculation that the pH of "normal" rainwater is about 5.7.

b) Scientists investigating acid rain measured the pH of a water sample from a lake and found it to be 4.8. The total concentration of dissolved carbonates in the lake is 4.5mmol/L. Determine the molar concentrations of the carbonate species CO3(2-), HCO3(-), and H2CO3 in the lake.

c) Suppose that 1 tonne(1t=10^3kg) of coal that is 2.5% sulfur by mass is burned in a coal-fired plant. What mass of SO2 is produced.

d) What is the pH of rainwater when the SO2 generated part c dissolves in a volume of water equivalent to 2 cm of rainfall over 2.6km^2 (the pKa1 of sulfurous acid is 1.81. Consider the water to be initially pure and at a pH of 7)

e)If the So2 in part c is first oxidized to SO3 before the rainfall, what would the pH of the same rainwater be?

f) one process used to clean SO2 from the emissions of coal-fired plants is to pass the stack gases along with air through a wet calcium carbonate slurry, where the following reaction will take place:

CaCO3s+SO2g+O2g--CaSO4s+CO2g

what mass of limestone (CaCO3) is needed to remove 50kg sulfur dioxide from stack gases if the removal process is 90% efficient?