If the coal is burned in a power plant that uses 2000 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide? How many grams of calcium sulfite are produced daily by this power plant?

Md Ariful Islam

0 like 0 dislike
1 views
Share with your friends

1 Answers

Md Ariful Islam

Call

$SO_2(g) + CaO(s) rarr CaSO_3(s)$

$"1 US ton"$ $=$ $907.19*kg$

$"Mass of coal(kg)"$ $=$ $2000*"ton"xx907*kg*"ton"^-1$ $=$ $1.814xx10^6*kg$.

$"Mass of sulfur"$ $=$ $1.814xx10^6*kgxx2.5%$ $=$ $45,350*kg$

$"Moles of sulfur"$ $=$ $(45,350*kgxx10^3*g*kg^-1)/(32.06*g*mol^-1)$ $=$ $1.41xx10^6*mol$.

And thus we may have $1.41xx10^6*mol$ $SO_2$ produced during the daily operation.

Given the equivalence of sulfur dioxide and calcium oxide in the first equation, clearly we need $1.41xx10^6*mol$ $CaO$ to produce $1.41xx10^6*mol$ $CaSO_3$.

$"Mass of calcium sulfite produced daily"$ $=$ $1.41xx10^6*molxx120.17*g*mol^-1$ $=$ $1.70xx10^8*g$ $=$ $1.70xx10^5*kg$.

There is a lot of arithmetic here; please go over my calculations; there is no money back guarantee.

0 like 0 dislike
1 views
Talk Doctor Online in Bissoy App
The recommended daily dose of calcium is 1200 mg. Calcium supplements often use calcium carbonate, $CaCO_3$, as the source of calcium. What mass of $CaCO_3$ should be used in a tablet so that one tablet provides the recommended daily dose of calcium?

$"Moles of calcium"$ $=$ $(1200xx10^-3*g)/(40.08*g*mol^-1)$ $=$ $0.04008*mol$. And thus we need $0.04008*mol$ $"calcium carbonate"$, i.e. a mass of $0.04008*molxx100.09*g*mol^-1$ $=$ $??g$.

1 Answers 1 views
If a $5.0*g$ mass of calcium carbonate is strongly heated to give a $2.8*g$ mass of calcium oxide, and a $2.2*g$ mass of carbon dioxide, how does this demonstrate the conservation of mass? How is this represented as an equation?

Is mass balanced in the given equation? We started with a mass of $5.0*g$ of calcium carbonate; from the reaction we get a mass of $2.8*g$ of oxide, and $2.2*g$...

1 Answers 1 views
How do you write an equation to represent "Calcium sulfite decomposes to form calcium oxide and sulfur dioxide"?

The first clue to go by is the fact that you're dealing with a , so you know that calcium sulfite is the only reactant and that you have two...

1 Answers 1 views
Decomposing calcium carbonate yields calcium oxide and dioxide. What information is needed to calculate the mass of calcium oxide that can produced from 4.7 kg of calcium carbonate?

The balanced chemical equation The molar mass of $"CaCO"_3$ The molar ratio of $"CaO"$ to $"CaCO"_3$ The molar mass of $"CaO"$ Your strategy has four steps:...

1 Answers 1 views
When propane, $C_3H_8$, is burned, carbon dioxide and water vapor are produced according to the following reaction: $C_3H_8 + 5O_2 -> 3CO_2 + 4H_2O$. How much propane is burned if 160.0 g of O2 are used and 132 g of CO2 and 72.0 g of H2O are produced?

$"Moles of carbon dioxide:"$ $(132*g)/(44.0*g*mol^-1)=3*mol$ $"Moles of water:"$ $(72*g)/(18.01*g*mol^-1)=4*mol$ $"Moles of oxygen:"$ $(160*g)/(32.0*g*mol^-1)=5*mol$ Because there were $3$ $mol$ carbon dioxide produced, and stoichiometric water, one mole precisely of propane was...

1 Answers 1 views
Calcium carbonate decomposes to form calcium oxide and carbon dioxide gas. If 44.5 grams of calcium oxide is produced, how many grams of calcium carbonate had to decomposez?

We need a stoichiometric reaction that represents the decomposition of calcium carbonate: $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ And thus calcium oxide and calcium carbonate are present in equimolar...

1 Answers 1 views
If you mixed 80 tons of sand, 12 tons of rock, and 4.0 tons of cement to make concrete, what would the percent by weight of sand be?

The mass percent of a component in a mixture is given by the formula $color(blue)(|bar(ul(color(white)(a/a) "Mass Percent" = "Mass of component"/"Mass of mixture" × 100 % color(white)(a/a)|)))" "$...

1 Answers 1 views
Iron (III) oxide reacts with carbon monoxide to form molten iron and carbon dioxide. If .18 g of iron (III) oxide reacts with 0.11 g of carbon monoxide, how many grams of iron would be produced?

$"Moles of ferric oxide "=(0.18*g)/(159.69*g*mol^-1)$ $=$ $1.13xx10^-3*mol" metal oxide"$. $"Moles of carbon monoxide "=(0.11*g)/(28.0*g*mol^-1)$ $=$ $3.93xx10^-3*mol" CO"$. $Fe_2O_3$ is the reagent in deficiency (why?), and thus $2xx1.13xx10^-3*molxx55.85*g*mol^-1~=0.150*g$ iron metal are...

1 Answers 1 views
Calcium oxide and carbon dioxide are produced from the decomposition of calcium carbonate. How many moles of calcium carbonate are needed to produce 15.0 grams of the calcium oxide?

We interrogate the stoichiometric equation...... $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g) uarr$ We require a molar quantity of $(15.0*g)/(56.08*g*mol^-1)=0.268*mol,$ with respect to $"calcium oxide"$. And clearly, we need a...

1 Answers 1 views
A mass of $2.40*g$ of calcium oxide is obtained by heating a mass of $5.00*g$ calcium carbonate. What is the stoichiometric equation that represents the formation of calcium oxide, and what is the percentage yield?

$CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ The $Delta$ symbol represents heat, and you have to fiercely heat these carbonates to effect decomposition. Note that this reaction is certainly stoichiometrically...

1 Answers 1 views
X