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Andrej [43]
2 years ago
8

Gaseous butano (CH,(CH),CH) will react with gaseous oxygen (0) to produce gaseous carbon dioxide (CO2) and goseous woter (11,0).

suppose
20.9 g of butane is mixed with 54, 9 of oxypen. Calculate the minimum mass of butone that could be left over by the chemical reaction. Be sure your answer
has the correct number of significant digits.
Chemistry
1 answer:
slega [8]2 years ago
5 0

Answer:

Firstly, We have to convert it in the Miles formula...

No. of moles = Mass given/Molar Mass

So, the final answer be come<em> </em>

<h3><em><u> </u></em><em><u>Ans</u></em><em><u> </u></em><em><u>-</u></em><em><u> </u></em><em><u>5</u></em><em><u>0</u></em><em><u>.</u></em><em><u>8</u></em><em><u> </u></em><em><u>gm</u></em><em><u> </u></em><em><u>and</u></em><em><u> </u></em><em><u>there</u></em><em><u> </u></em><em><u>same</u></em><em><u> </u></em><em><u>%</u></em><em><u> </u></em><em><u>is</u></em><em><u> </u></em><em><u>5</u></em><em><u>0</u></em><em><u>.</u></em><em><u>8</u></em><em><u>%</u></em><em><u> </u></em><em><u>butane</u></em><em><u> </u></em><em><u>in</u></em><em><u> </u></em><em><u>react</u></em><em><u>ion</u></em><em><u> </u></em></h3>
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During cellular respiration, plants take in _______ from the air and break down stored _______.
Zepler [3.9K]

Answer:

During cellular respiration, plants take in carbon dioxide from the air and break down stored glucose.

Explanation:

Before cellular respiration takes place in a plant, photosynthesis occurs and absorbs sunlight and carbon dioxide from the air. The process then produces oxygen and glucose, which are needed as the reactants for cellular respiration. Cellular respiration will break down the stored glucose to make energy to produce carbon dioxide and water. Then the cycle repeats itself.

7 0
3 years ago
Nitrogen dioxide is produced by combustion in an automobile engine. For the following reaction, 0.377 moles of nitrogen monoxide
Contact [7]

Answer:

The amount of NO₂ that can be produced 8.533 g

Explanation:

       According to question

                                2 NO(g) + O₂(g) → 2 NO₂(g)

Given

Moles of nitrogen monoxide = 0.377

Moles of oxygen = 0.278

'For NO'=\frac{Mole}{Stoichiometry}=\frac{0.377}{2} =0.1855\\'For O_{2} '=\frac{0.278}{1}= 0.278\\

Since 'NO' is the limiting reagent according to this ratio.

According to equation

         2 moles NO reacts to form 2 moles NO₂

So,  0.1855 moles NO give  = 0.1855 moles of NO₂

            Mass of 1 mole NO₂ = 46 g/mole

            Mass of 0.1855 moles = 46 x 0.1855 = 8.533 g

5 0
3 years ago
What do you think will happen to the Kool-Aid drink after it is boiled? CER(Claim,CITE evidence and reasoning) response THANK U
mafiozo [28]

Answer:

It is just sugar decomposing to a dark tar looking goo.

Explanation:

Cite: What happens after you boil kool-aid

4 0
2 years ago
Describe, on a molecular level, how you would expect these lipids to behave in water.
Gelneren [198K]
Lipids are hydrophobic; They would be insoluble, group together, and float to the top
7 0
3 years ago
A solution made by dissolving 33 mg of insulin in 6.5 mL of water has an osmotic pressure of 15.5 mmHg at 25°C. Calculate the mo
Liula [17]

<u>Answer:</u> The molar mass of the insulin is 6087.2 g/mol

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

\pi=iMRT

Or,

\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT

where,

\pi = osmotic pressure of the solution = 15.5 mmHg

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (insulin) = 33 mg = 0.033 g   (Conversion factor: 1 g = 1000 mg)

Volume of solution = 6.5 mL

R = Gas constant = 62.364\text{ L.mmHg }mol^{-1}K^{-1}

T = temperature of the solution = 25^oC=[273+25]=298K

Putting values in above equation, we get:

15.5mmHg=1\times \frac{0.033\times 1000}{\text{Molar mass of insulin}\times 6.5}\times 62.364\text{ L.mmHg }mol^{-1}K^{-1}\times 298K\\\\\text{molar mass of insulin}=\frac{1\times 0.033\times 1000\times 62.364\times 298}{15.5\times 6.5}=6087.2g/mol

Hence, the molar mass of the insulin is 6087.2 g/mol

8 0
3 years ago
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