All categories

2 years ago

Write 0.000 000 000 402 000 in scientific notation.

Chemistry

1 answer:

Rina8888 [55]2 years ago

4 0

Answer:

0.000000000402000 in scientific notation is 4.02000 × 10-10

You might be interested in

How do you calculate annual layers of snow from the past?

Zina [86]

It would be count ice layers

6 0

2 years ago

PLS HELP!! it’s science how do waves travel through gas

HACTEHA [7]

By 'waves' do you mean sound waves? If so sound waves need to travel through things like solids, liquids and yup gases. When the waves travel they are vibrating the molecules in the matter. By doing this he molecules in solids are packed very tightly.

6 0

2 years ago

What do you think would happen to a light bulb in the open circuit?

densk [106]

Is there choices to this question? cant answer it without choices

6 0

2 years ago

Choose the nonmetallic elements from the list. Check all that apply yttrium: oxygen: boron: polonium: argon: gallium: carbon:

BaLLatris [955]

Answer:

B, E, & G

Oxygen, Argon, & Carbon

7 0

3 years ago

Read 2 more answers

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