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3 years ago

Which is the coal with the highest energy available per unit to burn: lignite, subbituminous, bituminous, or anthracite?

Chemistry

1 answer:

olya-2409 [2.1K]3 years ago

6 0

Answer:

Anthracite

Explanation:

Anthracite produce highest amount of energy than other. It contain 86-97 percent carbon. Bituminous coal contain 45-86 percent carbon.

Subbituminous cola have 35-45 percent carbon while lignite contain 25-35 percent carbon.

Coal is source of many organic materials. It is fossil fuel and form after long period decay of plants. It is formed when trees are buried under earth

about 500 million years ago. The chemical and bacterial reactions take place and plant wood converted into the peat.

Than because of high temperature and pressure inside the earth peat is converted into the coal.

Through other processes it is than used to make the fuels such as coke. coal tar and coal gas.

Coal tar is the source of many organic compounds which are separated through fractional distillation.

About 80% of coal in Pakistan is used to bake the bricks and also used in lime kilns and for domestic purpose.

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Which of the following chemical equations is NOT correctly balanced?

forsale [732]

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3 years ago

Vitamin K is involved in normal blood clotting. When 0.802 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point

xenn [34]

Answer:

Molar mass of vitamin K = 450.56\frac{g}{mol}[/tex]

Explanation:

The freezing point of camphor = 178.4 ⁰C

the Kf of camphor = 37.7°C/m

where : m = molality

the relation between freezing point depression and molality is

Depression in freezing point = Kf X molality

Where

Kf = cryoscopic constant of camphor

molality = moles of solute dissolved per kg of solvent.

putting values

2.69°C = 37.7°C/m X molality

molality = 0.0714 mol /kg

$molality=\frac{molesofvitaminK}{massofcamphor(kg)}=\frac{moles}{0.025}$

moles of vitamin K = 0.0714X0.025 = 0.00178 mol

we know that moles are related to mass and molar mass of a substance as:

$moles=\frac{mass}{molarmass}$

For vitamin K the mass is given = 0.802 grams

therefore molar mass = $\frac{mass}{moles}=\frac{0.802}{0.00178}=450.56\frac{g}{mol}$

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3 years ago

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3 years ago

What is the molar mass of an unknown gas with a density of 2.00 g/L at 1.00 atm and 25.0 °C?

soldier1979 [14.2K]

Answer:

Explanation:Explanation:

Your starting point here will be the ideal gas law equation

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

∣

−−−−−−−−−−−−−−−

, where

- the pressure of the gas

- the volume it occupies

- the number of moles of gas

- the universal gas constant, usually given as

0.0821

atm

⋅

mol

⋅

- the absolute temperature of the gas

Now, you will have to manipulate this equation in order to find a relationship between the density of the gas,

, under those conditions for pressure and temperature, and its molar mass,

You know that the molar mass of a substance tells you the mass of exactly one mole of that substance. This means that for a given mass

of this gas, you can express its molar mass as the ratio between

and

, the number of moles it contains

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

∣

−−−−−−−−−−−−−

(

)

Similarly, the density of the substance tells you the mass of exactly one unit of volume of that substance.

This means that for the mass

of this gas, you can express its density as the ratio between

and the volume it occupies

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

∣

−−−−−−−−−−−

(

)

Plug equation

(

)

into the ideal gas law equation to get

⋅

Rearrange to get

⋅

Finally, use equation

(

)

to write

⋅

Convert the temperature of the gas from degrees Celsius to Kelvin then plug in your values to find

1.02

⋅

0.0821

atm

⋅

mol

⋅

(

273.15

)

0.990

atm

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

26.3 g mol

−

∣

−−−−−−−−−−−−−−−−

I'll leave the answer rounded to three

7 0

3 years ago