All of the following show a periodic pattern except

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

8090 [49]

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 $C_2H_6O_1N_2=C_2H_6ON_2$

8 0

4 years ago

What does ambitious mean?

Kobotan [32]

Answer:

Determination to succeed.

Explanation:

3 0

3 years ago

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An analytical chemist wants to measure the concentration of lead in drinking water in their building. They dilute 1mL of the sam

lidiya [134]

Answer:

b. 50ppm of Pb

c. 2x10⁻⁴M

j. no

Explanation:

The diluted sample has a concentration of 0.5 ppm of Pb. The sample was diluted from 1mL to 100mL. That means the dilution factor is:

100mL / 1mL = 100

That means, the sample was diluted 100 times from its original concentration.

As diluted sample has a concentration of 0.5ppm, the undiluted sample has a concentration of

0.5ppm×100 = 50ppm of Pb

1 ppm means 1x10⁻⁴ % by mass, 50 ppm are 50x10⁻⁴ % by mass

As molar mass of Pb is 207g/mol, molarity of 0.050g / L a(50 ppm) are:

0.050gₓ (1mol / 207g) / 1L = 2x10⁻⁴M

Based on EPA regulation, the maximum concentration of Lead in drinking water must be 0.015ppm. That means this water is not safe to drink

6 0

4 years ago

3.)

Luda [366]

Answer: Speed

Explanation:

8 0

3 years ago

What mass of glucose can be produced from a photosynthesis reaction that occurs using 10 moles of carbon dioxide?

BlackZzzverrR [31]

Hope this help. Answer will be on image.

6 0

4 years ago

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