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2 years ago

Need help with this chemistry homework

Chemistry

1 answer:

Elza [17]2 years ago

7 0

Answer:

10.0 ml and 35.0ml respectively

Explanation:

if A=10.0ml let B be x

Now,

Lets assume the pan is balanced

then,

x = 10.0 ml

Therefore B= 10.0 ml

[Repeat the same process in next question]

You might be interested in

Explain how the cell membrane controls the movement of materials into and out of the cell ?

sukhopar [10]

It's called simple diffusion, the small molecules without charges such as oxygen and carbon dioxide can flow through a plasma membrane without assistance and without expending energy. Other substances such as proteins, glucose and charged particles called ions cannot pass through the selectively permeable membrane.

5 0

2 years ago

Diamond is a natural form of pure carbon. What number of atoms of carbon are in a 1.00-carat diamond (1.00 carat = 0.200 g)?

slega [8]

Answer:

1.004×10²²

Explanation:

The molar mass of carbon is 12 g/mol

which means that:

1 mole of carbon atoms has a mass of 12 grams.

Since, diamond is a allotrope of carbon.

Mass of 1.00-carat diamond in grams is:

1.00 carat = 0.200 g

Since, 1 mole of C contains 6.022×10²³ atoms of C

So,

12 grams contains 6.022×10²³ atoms of C

1 gram contains 6.022×10²³/ 12 atoms of C

0.200 gram contains (6.022×10²³/ 12)×0.200 atoms of C

Thus,

1 carat diamond contains 1.004×10²² atoms of C.

8 0

2 years ago

Convert 5.28 x 1019 molecules of C6H1206 to grams.

nlexa [21]

Answer:

$m=0.0158g$

Explanation:

Hello there!

In this case, it is possible to comprehend these mass-particles problems by means of the concept of mole, molar mass and the Avogadro's number because one mole of any substance has 6.022x10²³ particles and have a mass equal to the molar mass.

In such a way, for C₆H₁₂O₆, whose molar mass is about 180.16 g/mol, the referred mass would be:

$m=5.28x10^{19}molecules*\frac{1mol}{6.022x10^{23}molecules}*\frac{180.16g}{1mol}\\\\m=0.0158g$

Best regards!

5 0

3 years ago

• 1) The pressure of a sample of gas in a 2.00-L container is 876 mmHg.

kifflom [539]

Answer:

4380 mmHg

Explanation:

Boyle's Law can be used to explain the relationship between pressure and volume of an ideal gas. The pressure is inversely related to volume, so if volume decrease the pressure will increase. It can be expressed in the equation as:

P1V1=P2V2

In this question, the first condition is 2L volume and 876 mmHg pressure. Then the system changed into the second condition where the volume is 400ml and the pressure is unknown. The pressure will be:

P1V1= P2V2

876 mmHg * 2L = P2 * 400ml /(1000ml/L)

P2= 876 mmHg * 2L / 0.4L

P2= 4380 mmHg

5 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]

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

Explanation:

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

2 years ago