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3 years ago

Which is the next logical step in balancing the given equation? CS2(1)+Cl2(g) CCl4(1) S2Cl2(1)

1 answer:

7 0

Reaction of current interest is:

CS2(l) + Cl2(g) → CCl4(l) + S2Cl2(l)

While balancing the chemical reaction, care must be taken that number of atoms of reactant side is equal to number of reactant on product side.

In present case, There is 1 'C' atom of both reactant and product side
There are 2 'S' atoms on both reactant and product side.
However, there are 2 Cl atoms of reactant side, but 6 Cl atoms on product side.
Hence multiplying Cl2 by 3, would equal the number of Cl atoms on both the sides.

Thus, the balanced reaction is
CS2(l) + 3 Cl2(g) → CCl4(l) + S2Cl2(l)

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3 years ago

mixture of N 2 And H2 Gases weighs 13.22 g and occupies a volume of 24.62 L at 300 K and 1.00 atm.Calculate the mass percent of

anygoal [31]

Answer: The mass percent of nitrogen gas and hydrogen gas is 91.41 % and 8.59 % respectively.

Explanation:

To calculate the number of moles, we use the equation given by ideal gas equation:

PV = nRT

where,

P = Pressure of the gaseous mixture = 1.00 atm

V = Volume of the gaseous mixture = 24.62 L

n = number of moles of the gaseous mixture = ?

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = Temperature of the gaseous mixture = 300 K

Putting values in above equation, we get:

$1.00atm\times 24.62L=n_{mix}\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 300K\\\\n_{mix}=\frac{1.00\times 24.62}{0.0821\times 300}=0.9996mol$

We are given:

Total mass of the mixture = 13.22 grams

Let the mass of nitrogen gas be 'x' grams and that of hydrogen gas be '(13.22 - x)' grams

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

For nitrogen gas:

Molar mass of nitrogen gas = 28 g/mol

$\text{Moles of nitrogen gas}=\frac{x}{28}mol$

For hydrogen gas:

Molar mass of hydrogen gas = 2 g/mol

$\text{Moles of hydrogen gas}=\frac{(13.22-x)}{2}mol$

Equating the moles of the individual gases to the moles of mixture:

$0.9996=\frac{x}{28}+\frac{(13.22-x)}{2}\\\\x=12.084g$

To calculate the mass percentage of substance in mixture we use the equation:

$\text{Mass percent of substance}=\frac{\text{Mass of substance}}{\text{Mass of mixture}}\times 100$

Mass of the mixture = 13.22 g

For nitrogen gas:

Mass of nitrogen gas = x = 12.084 g

Putting values in above equation, we get:

$\text{Mass percent of nitrogen gas}=\frac{12.084g}{13.22g}\times 100=91.41\%$

For hydrogen gas:

Mass of hydrogen gas = (13.22 - x) = (13.22 - 12.084) g = 1.136 g

Putting values in above equation, we get:

$\text{Mass percent of hydrogen gas}=\frac{1.136g}{13.22g}\times 100=8.59\%$

Hence, the mass percent of nitrogen gas and hydrogen gas is 91.41 % and 8.59 % respectively.

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3 years ago

200.00 grams of an organic compound is known to contain 83.884 grams of carbon, 10.486

Dmitriy789 [7]

Explanation:

Mass of the organic compound = 200g

Mass of carbon = 83.884g

Mass of hydrogen = 10.486g

Mass of oxygen = 18.640g

The mass of nitrogen = mass of organic compound - (mass of carbon + mass of hydrogen + mass of oxygen)

Mass of nitrogen = 200 - (83.884 + 10.486 + 18.64) = 200 - 113.01‬

Mass of nitrogen = 86.99g

The empirical formula of a compound is its simplest formula.

It is derived as shown below;

C H O N

Mass 83.884 10.486 18.64 86.99

molar

mass 12 1 16 14

Moles 83.884/12 10.486/1 18.64/16 86.99/14

6.99 10.49 1.17 6.21

Divide

lowest 6.99/1.17 10.49/1.17 1.17/1.17 6.21/1.17

6 9 1 5

Empirical formula C₆H₉ON₅

learn more:

Empirical formula brainly.com/question/2790794

#learnwithBrainly

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3 years ago

6. List the following particles in size order, from biggest to smallest?

Arte-miy333 [17]

Answer:

the particles, molecules, and gas range from smallest to largest in the following order: electron < proton < atom <...

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