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3 years ago

What is a limitation of using a chemical formula, such as CGH1206, to represent a compound?

Chemistry

1 answer:

Tpy6a [65]3 years ago

4 0

Answer:

The chemical formula does not show how the atoms are connected to one another.

Explanation:

With a chemical formula, you can see the types of elements that make up the compound, the number of atoms of each element in a molecule, and the chemical symbols of the elements in the compound.

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Sergio [31]

Answer:

C. The Protons

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3 years ago

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What kind of reaction is shown below?

MatroZZZ [7]

Answer:

d. decomposition

Explanation:

decomposition reaction is a reaction in which a compound breaks down into 2 or more substances.

the general form is: AB → A + B

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3 years ago

Who is generally credited with developing the process of using heat?

galina1969 [7]

Answer:

Robert Boyle

Explanation:

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2 years ago

If 2.1 moles of NaCl is dissolved in a solution with a total volume of 7.3 liters, what is the molarity of the solution? Round t

Arturiano [62]

Answer:

The molarity of the solution is 0.29 $\frac{moles}{liter}$

Explanation:

Molarity, or molar concentration, is a measure of the concentration of a solute in a solution, be it some molecular, ionic or atomic species. It is defined as the number of moles of solute that are dissolved in a given volume.

Molarity is calculated as the quotient between the number of moles of solutes and the volume of the solution:

$Molarity=\frac{number of moles of solute}{volume}$

Molarity is expressed in units $\frac{moles}{liter}$ .

In this case:

number of moles of solute= 2.1 moles
volume= 7.3 liters

Replacing:

$Molarity=\frac{2.1 moles}{7.3 liters}$

Molarity= 0.29 $\frac{moles}{liter}$

The molarity of the solution is 0.29 $\frac{moles}{liter}$

5 0

2 years ago

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Butane, C4H10, reacts with oxygen, O2, to form water, H2O, and carbon dioxide, CO2, as shown in the following chemical equation:

Wittaler [7]

The balanced chemical reaction is:

2C4H10(g)+13O2(g)->10H2O(g)+8CO2(g)

Calculate the mass of water produced when 1.77 grams of butane reacts with excessive oxygen?
1.77 g C4H10 (1 mol C4H10/58.14 g C4H10) (10 mol H2O / 2 mol C4H10) ( 1.01 g H2O / 1 mol H2O ) = 0.15 g H2O

Calculate the mass of butane needed to produce 71.6 of carbon dioxide.
71.6 g CO2 (1 mol CO2/ 44.01 g CO2) ( 2 mol C4H10 / 8 mol CO2 ) (58.14 g C4H10 / 1 mol C4H10 ) = 23.65 g C4H10

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3 years ago

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