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3 years ago

What is the empirical formula for C2H6?

2 answers:

7 0

The empirical formula is a formula obtained as the result of the quantitative analysis.

СH₃ is the empirical formula for C₂H₆

finlep [7]3 years ago

4 0

Answer:

Empirical formula for $C_{2}H_{6}$ is $CH_{3}$

Explanation:

Empirical formula of a molecule contains symbol of all constituent atoms along with their lowest possible stoichiometric coefficient.

In $C_{2}H_{6}$ , stoichiometric coefficients of C and H are 2 and 6 respectively.

We can write this formula as - $(CH_{3})_{2}$

So clearly the lowest possible stoichiometric coefficients of C and H would be 1 and 3 respectively.

So empirical formula is $CH_{3}$

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Can You Tell? Pepsinogen is released in the stomach. Why can't it digest stomach walls?

miv72 [106K]

Answer:

Specific cells within the gastric lining, known as chief cells, release pepsin in an inactive form, or zymogen form, called pepsinogen. By doing so, the stomach prevents the auto-digestion of protective proteins in the lining of the digestive tract.

Explanation:

Make sure to edit so you don't get copy-writed

5 0

3 years ago

A 0.216 g sample of carbon dioxide, CO2, has a volume of 507 mL and a pressure of 470 mmHg. What is the temperature of the gas i

Gala2k [10]

Answer:

The temperature of the gas is 876.69 Kelvin

Explanation:

Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P*V = n*R*T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.

In this case:

P= 470 mmHg
V= 570 mL= 0.570 L
n= 0.216 g= 0.0049 moles (being the molar mass of carbon dioxide is 44 g/mole)

R= 62.36367 $\frac{mmHg*L}{mol*K}$

Replacing:

470 mmHg*0.570 L= 0.0049 moles* 62.36367 $\frac{mmHg*L}{mol*K}$ *T

Solving:

$T=\frac{470 mmHg*0.570 L}{0.0049 moles* 62.36367\frac{mmHg*L}{mol*K} }$

T= 876.69 K

The temperature of the gas is 876.69 Kelvin

6 0

2 years ago

how much hydrogen will be released during the interaction of potassium weighing 8 grams with hydrochloric acid

krek1111 [17]

Answer:

With an understanding of the ideal gas laws, it is now possible to apply these principles to chemical stoichiometry problems. For example, zinc metal and hydrochloric acid (hydrogen chloride dissolved in water) react to form zinc (II) chloride and hydrogen gas according to the equation shown below:

2 HCl (aq) + Zn (s) → ZnCl2 (aq) + H2 (g)

Explanation:

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$\large\colorbox{lightblue}{Xxᴊᴀsʜ13xX}$

4 0

2 years ago

An organic molecule is likely to contain all of these elements except: Answer C H O Ne N

eimsori [14]

Organic molecules typically do not contain the noble gases, so they would contain all but Ne

8 0

3 years ago

What mass of radon is in 8.17 moles of radon?

Len [333]

Answer:

1813.74g

Explanation:

Given parameters:

Number of moles of radon = 8.17moles

Unknown:

Mass of radon = ?

Solution:

To solve this problem, we use the expression below:

Number of moles = $\frac{mass}{molar mass}$

Molar mass of radon = 222g/mol

Now insert the parameters and solve;

Mass of radon = Number of moles x molar mass

= 8.17 x 222

= 1813.74g

4 0

3 years ago