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2 years ago

How many Liters of H2O are in 1.50 g H2O?

Chemistry

2 answers:

zlopas [31]2 years ago

6 0

Answer:18.02 grams

The average mass of one mole of H2O is 18.02 grams.

Explanation: we need to find the moles of water in 1 L of water or 1000mL of water. Taking the density of water to be 1g/mL, 1000mL of water= 1000g water.

Therefore, number of moles= given mass of water(1000)/molecular mass of water(18)

Moles =1000/18= 55.55

So total molecules in 55.55 moles= 55.55* 6.022*10^23 = 334.52*10^23 molecules

=3.34*10^25 molecules of water.

Trava [24]2 years ago

6 0

Answer:

18.02

Explanation:

is your answer

<h2><u>PLZ mark me as a Brainliest</u></h2>

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A solution of naoh(aq) contains 8.1 g of naoh(s) per 100.0 ml of solution. calculate the ph and the poh of the solution at 25 °c

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2 years ago

Titanium has an HCP unit cell for which the ratio of the lattice parameters c/a is 1.58. If the radius of the Ti atom is 0.1445

Karolina [17]

The unit cell volume of the crystal is $V_c = 9.9084*10^-^2^3 cm^3 / unit cell$ and the density of titanium is calculated as 4.71g/cm^3 while the literature value is 4.5 g/cm^3

Data;

radius = 0.1445 nm
c/a = 1.58
A = 46.88 g/mol

<h3>Unit Cell Volume</h3>

The unit cell volume can be calculated as

$V_c = 6R^2c\sqrt{3}\\$

let's substitute the values into the formula

$V_c = 6 * (1.445*10^-^8)^2 * 1.58 8 * a * \sqrt{3} \\a = 2R\\V_c = 6 * (1.445*10^-^8)^2 * 1.58* 2 * 1.445*10^-^8 * \sqrt{3}\\ V_c = 9.984*10^-^2^3 cm^3 / unit cell$

The unit cell volume of the crystal is $V_c = 9.9084*10^-^2^3 cm^3 / unit cell$

<h3>Density of Ti</h3>

The density of titanium can be calculated as

$\rho = \frac{nA}{V_c N_a}$

n = 6 for hcp
A = 46.88 g/mol
Na = Avogadro's number

let's substitute the values into the formula

$\rho = \frac{nA}{V_c Na}\\ \rho = \frac{6*46.88}{9.9084*10^-^2^3* 6.023*10^2^3} \\\rho = 4.71 g/cm^3$

The density of titanium is calculated as 4.71g/cm^3 while the literature value is 4.5 g/cm^3

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2 years ago

What are the resonance structures of the<br>carbonate (CO32-) ion?

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Answer:

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Explanation:

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2 years ago

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Answer:

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2 years ago

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What is the pressure of a sample of gas at a volume of .335 L if it occupies 1700 mL at

Alchen [17]

Answer:

4,313.43 mmHg is the pressure of a sample of gas at a volume of .335 L if it occupies 1700 mL at 850 mm Hg

Explanation:

Boyle's law says:

"The volume occupied by a given gas mass at constant temperature is inversely proportional to the pressure." This means that if the quantity of gas and the temperature remain constant, the product of the pressure for the volume always has the same value.

Boyle's law is expressed mathematically as:

Pressure * Volume = constant

o P * V = k

If you have a certain volume of gas V1 that is at a pressure P1 at the beginning of the experiment and you vary the volume of gas to a new value V2, then the pressure will change to P2, it will be true:

P1 * V1 = P2 * V2

In this case:

V1=0.335 L
P1= ?
V2= 1700 mL= 1.7 L (Being 1 L=1000 mL)
P2= 850 mmHg

Replacing:

P1*0.335 L=850 mmHg*1.7 L

Solving:

$P1=\frac{850 mmHg*1.7 L}{0.335 L}$

<u><em>4,313.43 mmHg is the pressure of a sample of gas at a volume of .335 L if it occupies 1700 mL at 850 mm Hg</em></u>

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2 years ago