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spin [16.1K]
2 years ago
8

PLS HELPP DUE TODAY NEED DONE

Chemistry
2 answers:
Zarrin [17]2 years ago
3 0

Answer:

Explanation:

Each coil increases it by a multiple of 100.

=> 50 | 3 | <u><em>15,000</em></u>

=> 100 | 3 | <u><em>30,000</em></u>

=> 150 | 3 | <u><em>45,000</em></u>

IgorC [24]2 years ago
3 0
Ha that's rlly sad imagine having this die today lol
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What compound is this?
Nezavi [6.7K]

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Carbon Tetrachloride

Explanation:

1 Carbon atom, 4 chlorine atoms (hence "tetra" prefix)

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For the following SN1 solvolysis reaction, select the correct rate equation and the overall reaction order (note: CH3OH is the s
sineoko [7]

Answer:

Explanation:

  • rate = K[(CH3)3CCl]
  • overall order is also first order

Since we are told that CH3OH is the solvent for the reaction, as such the rate law equation will only be written for (CH3)3CCl .

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Ep-15 why is carbon monoxide especially dangerous?
Rzqust [24]

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8 0
2 years ago
Ammonia and oxygen react to form nitrogen and water.
Nata [24]

Answer:

A. 19.2 g of O2.

B. 3.79 g of N2.

C. 54 g of H2O.

Explanation:

The balanced equation for the reaction is given below:

4NH3(g) + 3O2(g) → 2N2+ 6H2O(g)

Next, we shall determine the masses of NH3 and O2 that reacted and the masses of N2 and H2O produced from the balanced equation.

This is illustrated below:

Molar mass of NH3 = 14 + (3x1) = 17 g/mol

Mass of NH3 from the balanced equation = 4 x 17 = 68 g

Molar mass of O2 = 16x2 = 32 g/mol

Mass of O2 from the balanced equation = 3 x 32 = 96 g

Molar mass of N2 = 2x14 = 28 g/mol

Mass of N2 from the balanced equation = 2 x 28 = 56 g

Molar mass of H2O = (2x1) + 16 = 18 g/mol

Mass of H2O from the balanced equation = 6 x 18 = 108 g

Summary:

From the balanced equation above,

68 g of NH3 reacted with 96 g of O2 to produce 56 g of N2 and 108 g of H2O.

A. Determination of the mass of O2 needed to react with 13.6 g of NH3.

This is illustrated below:

From the balanced equation above,

68 g of NH3 reacted with 96 g of O2.

Therefore, 13.6 g of NH3 will react with = (13.6 x 96)/68 = 19.2 g of O2.

Therefore, 19.2 g of O2 are needed for the reaction.

B. Determination of the mass of N2 produced when 6.50 g of O2 react.

This is illustrated below:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Therefore, 6.5 g of O2 will react to produce = (6.5 x 56)/96 = 3.79 g of N2.

Therefore, 3.79 g of N2 were produced from the reaction.

C. Determination of the mass of H2O formed from the reaction of 34 g of NH3.

This is illustrated below:

From the balanced equation above,

68 g of NH3 reacted to 108 g of H2O.

Therefore, 34 g of NH3 will react to produce = (34 x 108)/68 = 54 g of H2O.

Therefore, 54 g of H2O were obtained from the reaction.

4 0
2 years ago
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