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SCORPION-xisa [38]
2 years ago
9

Ethanol is being used as an additive to

Chemistry
1 answer:
CaHeK987 [17]2 years ago
3 0

Answer:

1.Begin energy in kilojoules.

2.Use a conversion factor in convert kilojoules to joules .

3.Use a conversion factor top convert

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QUESTION 21 The combustion of ammonia in the presence of excess oxygen yields NO 2 and H 2O: 4 NH 3 (g) 7 O 2 (g) 4 NO 2 (g) 6 H
Harrizon [31]

Answer:

The answer to your question is 47.44 g of Oxygen

Explanation:

Data

mass of Ammonia = 14.4 g

mass of Oxygen = ?

Balanced chemical reaction

                 4NH₃  +  7O₂  ⇒  4NO₂  +  6H₂O

Process

1.- Calculate the molar mass of Ammonia

NH₃ = 4[(1 x 14) + (3 x 1)] = 4[14 + 3] = 4[17] = 68 g

2.- Calculate the molar mass of Oxygen

O₂ = 7[16 x 2] = 7[32] = 224 g

3.- Use proportions to calculate the mass of Oxygen

                     68g of NH₃ --------------------- 224 g of O₂

                      14.4 g of NH₃ -----------------  x

                       x = (14.4 x 224) / 68

                       x = 3225.6/ 68

                       x = 47.44 g

5 0
3 years ago
If you dilute 40.0 mL of a 7.0 M solution to make 100.0 mL of solution, what is the molarity of the dilute solution?
Burka [1]

Answer:

2.8M

Explanation:

The following data were obtained from the question:

Volume of stock solution (V1) = 40mL

Molarity of the stock solution (M1) = 7M

Volume of diluted solution (V2) = 100mL

Molarity of diluted solution (M2) =?

Using the dilution formula, we can easily find the molarity of the diluted solution as follow:

M1V1 = M2V2

7 x 40 = M2 x 100

Divide both side by 100

M2 = (7 x 40)/100

M2 = 2.8M

Therefore, the molarity of the diluted solution is 2.8M

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What are two examples of an endothermic reaction and what are two examples of an ectothermic reaction?
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Exothermic processes: Making ice cubes,formation of snow in clouds


Endothermic processe: Melting ice cubes, evaporation of water
7 0
4 years ago
Bonds in which atoms share electrons are defined as _____ bonds.
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Ionic, think about the way metals share electrons with other metals, resulting in malleability.
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