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2 years ago

Which of the following is an empirical formula? H6O2 H402 H2O H2O2

Chemistry

2 answers:

Jobisdone [24]2 years ago

6 0

Answer:

hola responderé

Explanation:

el h2o es agua y el agua es mojada gracias por su atención

topjm [15]2 years ago

5 0

${\qquad\qquad\huge\underline{{\sf Answer}}}$

<h3>What does an empirical formula mean ? </h3>

- Empirical formula represents a molecule with its elements combined in simplest ratio, it's not necessarily same as the form in which the compound really exists in the nature. Hence we can say that empirical formula shows the simple ratios in which atoms combined to form a molecule.

For example : Hydrogen peroxide

- Hydrogen peroxide exists in nature as $\sf H_2O_2$ , which is its molecular formula.

but it's empirical formula will be H0 [ simplest ratio of 1 : 1 ]

Therefore, the correct choice is :

C. $\sf H_2O$

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The correct answer is (1) one mole of NO2.

The gram formula mass is also known as the molar mass and is defined by the mass over one mole of a substance.

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3 years ago

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Explain why a solution has a lower boiling point than the pure solvent

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Because the intention is to boil the solution, the purpose of the solvent is to dissolve so it has a higher boiling point so ensure it stays in liquid form and doesn't evaporate into a gas

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4 years ago

A 7.0 g sample of a hydrocarbon (a molecule that has only hydrogen and carbon) is subject to combustion analysis. The mass of CO

Akimi4 [234]

Answer: The empirical formula for the given compound is $CH_2$

Explanation:

The chemical equation for the combustion of compound having carbon and hydrogen follows:

$C_xH_y+O_2\rightarrow CO_2+H_2O$

where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.

We are given:

Mass of $CO_2=22.0g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 22.0 g of carbon dioxide, $\frac{12}{44}\times 22.0=6g$ of carbon will be contained.

For calculating the mass of hydrogen:

Mass of hydrogen = Mass of sample - Mass of carbon

Mass of hydrogen = 7.0 g - 6 g

Mass of hydrogen = 1.0 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{6g}{12g/mole}=0.5moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1.0g}{1g/mole}=1.0moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.5 moles.

For Carbon = $\frac{0.5}{0.5}=1$

For Hydrogen = $\frac{1.0}{0.5}=2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of Fe : C : H = 1 : 2

Hence, the empirical formula for the given compound is $C_{1}H_{2}=CH_2$

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4 years ago

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Answer:

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Absolute temperature refers to the lowest possible temperature. At this state, no heat energy remains in the substance; the energy of the particles are at their lowest energy points.

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