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3 years ago

What is not represented by a balanced chemical equation?

Chemistry

2 answers:

Vladimir [108]3 years ago

7 0

The correct answer is:

B) The same subscripts are on each side of the equation.

katrin [286]3 years ago

3 0

Answer: The correct answer is Option B.

Explanation:

A balanced chemical equation follows law of conservation of mass.

This law states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form. This means that total mass on the reactant side is equal to the total mass on the product side.

This also means that the total number of individual atoms on the reactant side will be equal to the total number of individual atoms on the product side.

For Example: Reaction of hydrochloric acid with sodium hydroxide, the equation follows:

$HCl+NaOH\rightarrow NaCl+H_2O$

From the above chemical equation, the chemical formula for the substances are written correctly on both the sides of the reaction. But the subscript of hydrogen on the reactant side is 1 and on the product side is 2.

Thus, the correct answer is Option B.

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Hunter-Best [27]

The statement above is FALSE.

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3 years ago

Asap... define pure substances...

gtnhenbr [62]

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3 years ago

Read 2 more answers

A 1.68 g sample of water is injected into a closed evacuated 5.3 liter flask at 65°C. What percent (by mass) of the water will b

Angelina_Jolie [31]

Answer:

50.4 % of the water will be vapor

Explanation:

Step 1: Data given

Mass of water = 1.68 grams

volume of the flask = 5.3 L

Temperature = 65°C

Vapor pressure of water at 65°C = 187.5 mmHg = 0.2467 atm

Step 2: Calculate moles of H2O

p*V=n*R*T

⇒ p = the pressure of water = 0.2467 atm

⇒ V = the volume of the flask = 5.3 L

⇒ n = moles of water

⇒ R = gas constant = 0.08206 L*atm/ K*mol

⇒ T = the temperature = 65°C = 338 Kelvin

n = (p*V)/(R*T)

n = (0.2467 * 5.3) /(0.08206* 338)

n = 0.047 moles

Step 3: Calculate mass of water

Mass of water = moles of water * molar mass of water

Mass of water = 0.047 moles *18.02 g/mol

Mass of water = 0.84694 grams

Step 4: Calculate the percent of water vaporized

% = (0.84694 grams/1.68 grams) *100%

% = 50.4%

50.4 % of the water will be vapor

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Rainbow [258]

Answer:

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Explanation:

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If I added 50 grams of salt to water and evaporated the solution with a hot plate, what amount of salt would be left behind?

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