How many grams of calcium sulfite are produced daily by this power plant?

Explanation:

Explanation:

S

O

2

(

g

)

+

C

a

O

(

s

)

→

C

a

S

O

3

(

s

)

1 US ton

=

907.19

⋅

k

g

Mass of coal(kg)

=

2000

⋅

ton

×

907

⋅

k

g

⋅

ton

−

1

=

1.814

×

10

6

⋅

k

g

.

Mass of sulfur

=

1.814

×

10

6

⋅

k

g

×

2.5

%

=

45

,

350

⋅

k

g

Moles of sulfur

=

45

,

350

⋅

k

g

×

10

3

⋅

g

⋅

k

g

−

1

32.06

⋅

g

⋅

m

o

l

−

1

=

1.41

×

10

6

⋅

m

o

l

.

And thus we may have  

1.41

×

10

6

⋅

m

o

l

S

O

2

produced during the daily operation.

Given the equivalence of sulfur dioxide and calcium oxide in the first equation, clearly we need  

1.41

×

10

6

⋅

m

o

l

C

a

O

to produce  

1.41

×

10

6

⋅

m

o

l

C

a

S

O

3

.

Mass of calcium sulfite produced daily

=

1.41

×

10

6

⋅

m

o

l

×

120.17

⋅

g

⋅

m

o

l

−

1

=

1.70

×

10

8

⋅

g

=

1.70

×

10

5

⋅

k

g

.

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).

a is the correct answer