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4 years ago

3. What is the volume of 0.750 mol of argon at STP?

Chemistry

1 answer:

Zepler [3.9K]4 years ago

3 0

Answer:

The volume is 16.7 liters.

Explanation:

STP conditions are:

1 atm as pressure

273 K as temperature (0°C)

So let's get the volume by the Ideal Gas Law, replacing the values.

P . V = n . R . T

1 atm . V = 0.750 moles . 0.082 L.atm /mol.K . 273 K

V = (0.750 moles . 0.082 L.atm /mol.K . 273 K) / 1 atm

V = 16.7 L

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. Dimethyl nitrosamine is a known carcinogen. It can be formed in the intestinal tract when digestive juices react with the nitr

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Answer: The empirical formula for the given compound is $C_2H_6ON_2$

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

$C_xH_yN_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and nitrogen respectively.

We are given:

Mass of $CO_2=5.134g$

Mass of $H_2O=3.173g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

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

So, in 5.134 g of carbon dioxide, $\frac{12}{44}\times 5.134=1.4g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 3.173 g of water, $\frac{2}{18}\times 3.173=0.35g$ of hydrogen will be contained.

For calculating the mass of nitrogen:

As, 100 g of sample contains 37.87 % of nitrogen

So, 4.319 g of sample contains $\frac{37.87}{100}\times 4.319=1.635g$ of nitrogen

For calculating the mass of oxygen:

Mass of oxygen in the compound = (4.319) - (1.4 + 0.35 + 1.635) = 0.934 g

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

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{1.4g}{12g/mole}=0.116moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.35g}{1g/mole}=0.35moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.934g}{16g/mole}=0.058moles$

Moles of Nitrogen = $\frac{\text{Given mass of nitrogen}}{\text{Molar mass of nitrogen}}=\frac{1.635g}{14g/mole}=0.116moles$

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 0.058 moles.

For Carbon = $\frac{0.116}{0.058}=2$

For Hydrogen = $\frac{0.35}{0.058}=6.03\approx 6$

For Oxygen = $\frac{0.058}{0.058}=1$

For Oxygen = $\frac{0.116}{0.058}=2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O : N = 2 : 6 : 1 :2

Hence, the empirical formula for the given compound is $C_2H_6O_1N_2=C_2H_6ON_2$

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4 years ago

Which of these statements is true? A. Some molecules may contain no atoms. B. Some elements found in nature exist as molecules.

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I think it is most likely B. Some elements found in nature exist as molecules. Like for instance the element of oxygen. We can think of it in nature as a diatomic molecule,

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Not always ammonium salts of weak acids form neutral solutions.

When formic acid reacts with ammonia, ammonium formate is produced:

HCO2H + NH3 ----> NH4HCO2

You already know that the weak conjugate bases of NH3 and HCO2H are NH4+ and HCO2, respectively.

How can the pH of the solution be calculated if the salt's anion causes the pH to rise and the salt's cation causes it to fall? The relative intensities of the basic anion and the acidic cation hold the key to the solution.

As was already established, formate is a weak base and will create hydroxide ions in water, whereas ammonium is a weak acid and will make hydronium ions in water.

NH4⁺ + H2O -----> NH3 + H3O⁺

HCO2⁻ + H2O -----> HCO2H + OH⁻

Since the acid ionization of NH4+ is more favored than the base ionization of HCO2-, the solution will be acidic.

To learn more about ammonium salts:

brainly.com/question/10874844

#SPJ4

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2 years ago

3. What is the volume of 0.750 mol of argon at STP?​

3. What is the volume of 0.750 mol of argon at STP?