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Phoenix [80]
3 years ago
6

Which of the following is an example of a reaction that you've seen in your everyday life ?

Chemistry
2 answers:
Feliz [49]3 years ago
8 0

Answer:

ice melting

Explanation:

soldier1979 [14.2K]3 years ago
7 0
I believe this pertains to chemical reaction? So my guess would be answer A “Fire burning”

Don’t quote me though lol.
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The volume of 7.91 M HCl needed to make 196.1 mL of 2.13 M HCl is ____.
kumpel [21]

Answer:

a) 52.8

Explanation:

M1V1 = M2V2

(7.91 M)(x ml) = (2.13 M) (196.1 ml)

(7.91M) (xml) = 417.693 M.ml

x ml = 417.693/ 7.91

x   =  52.8

6 0
3 years ago
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This equation shows the combustion of methanol.
sveticcg [70]

Answer: 44.8 L

Explination:

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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
Which of these is the strongest acid?
sergejj [24]

Answer: D

Explanation:

8 0
3 years ago
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50.0 grams of KCl is dissolved in water to make a 4.00 L
xeze [42]

Answer:0.1677M

Explanation:

Molarity=moles/volume

Number of moles =mass/molar mass

Once you get the number of moles, you apply it to the molarity formula.

8 0
3 years ago
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