Ask question

Ask question

All categories

2 years ago

9

What would be the mass of 4.56x10²³ water molecules

1 answer:

kifflom [539]2 years ago

3 0

Every time you see molecules, atoms, & particles think of avagadros #. (6.022 x 10^23)

Answer: 13.6 grams of H2O

Solution: (4.56x10^23) x (1 mol H2O/6.022x10^23) x (18 grams H2O/1 mol H2O) = 13.6 grams of H2O

Using dimensional analysis above makes these types of problems easy.

You might be interested in

Why is a bannana curved?

Yanka [14]

Answer:

Explanation:

It's because of the sun! Bananas are curved so they can retrieve sunlight.

7 0

2 years ago

Read 2 more answers

How many electrons in the same atom can share the quantum number n = 2?

melisa1 [442]

With the principle quantum number being 2, the maximum number that can share this is 8. You can use the general formula 2n^2 to calculate this number (n=quantum level), or you can use the concept of quantum numbers (n, l, m, s) to justify this answer.

3 0

2 years ago

Cryogenics has the potential to be useful in a variety of fields, including medicine. Suppose you have engineered a method to su

tatiyna

Explanation:

It is known that the specific heat capacity of Liver $(C_{p})$ is 3.59 kJ $kg^{-1}.K^{-1}$

It is given that :

Initial temperature of Liver = Body temperature = $37^{o}C$ = 310 K

Final temperature of Liver = 180 K

Relation between heat energy, mass, and change in temperature is as follows.

Q = $m \times C_{p} \times \Delta T$

Now, putting the given values into the above formula as follows.

Q = $m \times C_{p} \times \Delta T$

Q = $1.5 kg \times 3.59 kJ/kg.K \times (310 - 180) K$

= 700.05 kJ

Therefore, we can conclude that amount of heat which must be removed from the liver is 700.05 kJ.

7 0

3 years ago

The molar mass of H2O is 18.01 g/mol. The molar mass of O2 is 32.00 g/mol. What mass of H2O, in grams, must react to produce 50.

snow_lady [41]

112.5 g. The production of 50.00 g O2 requires 112.5 g H2O.

a) Write the partially balanced equation for the decomposition of water.

MM = 18.02 32.00

2H2O → O2 + …

Mass/g = 50.00

b) Calculate the <em>moles of O2
</em>

Moles of O2 = 50.00 g O2 × (1 mol O2/16.00 g O2) = 3.1250 mol O2

c) Calculate the <em>moles of water</em>

Moles of H2O = 3.1250 mol O2 × (2 mol H2O/1 mol O2)

= 6.2500 mol H2O

d) Calculate the mass of water

Mass of H2O = 6.2500 mol H2O × (18.02 g H2O/1 mol H2O)

= 112.5 g H2O

5 0

2 years ago

A gas has a pressure of 1.34 atm when the temperature is 237K. The gas is then heated until the temperature measures 312K. What

alexandr1967 [171]

The answer for the following question is answered below.

<em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>

Explanation:

Given:

Initial pressure of the gas = 1.34 atm

Initial temperature of the gas = 273 K

final temperature of the gas = 312 K

To solve:

Final temperature of the gas

We know;

From the ideal gas equation

P × V = n × R × T

So;

from the above equation we can say that

<em>P ∝ T</em>

$\frac{P}{T}$ = constant

$\frac{P_{1} }{P_{2} }$ = $\frac{T_{1} }{T_{2} }$

Where;

$P_{1}$ = initial pressure of a gas

$P_{2}$ = final pressure of a gas

$T_{1}$ = initial temperature of a gas

$T_{2}$ = final temperature of a gas

$P_{2}$ = $\frac{1.34*312}{237}$

$P_{2}$ = 1.76 atm

<em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>

6 0

3 years ago