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Inessa05 [86]
3 years ago
7

Acid rain can be destructive to both the natural environment and human-made structures. The equation below shows a reaction that

occurs that may lead to the formation of acid rain. 3NO2 + H2O mc025-1.jpg 2HNO3 + NO How many moles (precise to the nearest 0.01 mol) of nitric acid are produced from 300.00 mol of nitrogen dioxide?
Chemistry
2 answers:
alexandr1967 [171]3 years ago
8 0
The moles of nitric acid formed can be computed using the stoichiometric relation obtained from the given equation which indicates that for every 3 moles of nitrogen dioxide (NO2), 2 moles of nitric acid (HNO3) is formed. 300 moles of NO2 is then multiplied to 2 mol HNO3/ 3 mol NO2. The answer is 200 moles of nitric acid is produced from 300 moles of NO2. 
VLD [36.1K]3 years ago
4 0

Answer;

200.00 moles of nitric acid is produced

Explanation;

From the equation;

3NO2 + H2O → 2HNO3 + NO

The mole ratio of nitrogen (IV) oxide  and nitric acid is 3 is to 2;

Thus; for every 3 moles of nitrogen dioxide (NO2), 2 moles of nitric acid (HNO3) are formed. 

Therefore; 300 moles of NO2 will produce;

2 mol HNO3/ 3 mol NO2 (300) = 200 moles

Hence, 200 moles of nitric acid are produced from 300 moles of NO2. 

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A chemical reaction can be reversed if?
Wittaler [7]

Chemical reaction can be reversed if the energy of the reactants is less than the activation energy threshold.

<h3>What is a reversible reaction?</h3>

A reversible reaction is a reaction in which the conversion of reactants to products and the conversion of products to reactants occur simultaneously.

<h3>Conditions for reversible reaction</h3>

In equilibrium reaction, the activation energy of the forward reaction is more than that of backward reaction which causes bond breakage of the reactants.

Activation energy = (Threshold energy) - (Internal energy of the reactants)

Thus, a chemical reaction can be reversed if the energy of the reactants is less than the activation energy threshold.

Learn more about reversible reaction here: brainly.com/question/16614855

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4 0
1 year ago
Name physical properties
Paraphin [41]

Answer:

<u>Some examples of physical properties are: </u>

color (intensive)

density (intensive)

volume (extensive)

mass (extensive)

boiling point (intensive): the temperature at which a substance boils.

melting point (intensive): the temperature at which a substance melts.

Explanation:

Hope this helped! <3

8 0
3 years ago
Which is an example of what should be done in case of a laboratory accident? Wear appropriate lab attire. Read directions comple
riadik2000 [5.3K]

Answer: C. Do not try to clean up a spill.

Explanation:

6 0
3 years ago
Read 2 more answers
What is the mass in grams of 0.375 mol if the element potassium, k?<br><br>​
alexandr402 [8]

Answer: 14.625g

Explanation:

No of moles= mass given/molar mass

No of moles given= 0.375mol

Mass is the unknown (?)

Molar mass of K= 39

No of moles = mass given/molar mass

Substitute the values

0.375= mass/39

Cross multiply

Mass = 39×0.375

Mass= 14.625g

The mass is 14.625g

3 0
3 years ago
Read 2 more answers
A standard lanthanum solution is prepared by dissolving 0.1968 grams of lanthanum oxide (La2O3) in excess nitric acid and diluti
sweet-ann [11.9K]

Answer:

1.208x10⁻³M and 392.5ppm La(NO3)3

Explanation:

The reaction that occurs is:

La2O3 + 6HNO3 → 2La(NO3)3 + 3H2O

Molarity is defined as the moles of solute (In this case, LaO3) per liter of solution. And ppm, are mg of solute per liter of solution.

To solve this question we must find the moles of La(NO3)3 produced and its mass in milligrams to find molarity and ppm:

<em>Moles La2O3 -Molar mass: 325.81g/mol-</em>

0.1968g * (1mol / 325.81g) = 6.04x10⁻⁴ moles La2O3

<em>Moles La(NO3)3:</em>

6.04x10⁻⁴ moles La2O3 * (2mol La(NO3)3 / 1mol La2O3) = 1.208x10⁻³ moles La(NO3)3

<em>Molarity:</em>

1.208x10⁻³ moles La(NO3)3 / 1L =

<h3>1.208x10⁻³M</h3>

<em>Mass La(NO3)3 -Molar mass: 324.92g/mol-</em>

1.208x10⁻³ moles La(NO3)3 * (324.92g / mol) = 0.392.5g La(NO3)3

In mg:

392.5mg La(NO3)3 / 1L =

392.5ppm La(NO3)3

7 0
2 years ago
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