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2 years ago

I NEED HELP ASAP !!!!!!!!!!!!!!!!!!!!!1

Chemistry

1 answer:

Karolina [17]2 years ago

6 0

Answer:

true im pretttyyy sure

Explanation:

bcuz the stronger the intermolecular forces the higher the boiling point :3

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Iron(II) is available to bond with chloride ion. How many of each type of ion will bond to form an ionic compound?

Evgesh-ka [11]

Answer:

D) 1 iron(II), 2 chloride

Explanation:

Iron II chloride is the compound; FeCl2. It is formed as follows, ionically;

Fe^2+(aq) + 2Cl^-(aq) -----> FeCl2

The formation of one mole of FeCl2 involves the reaction one mole of iron and two moles of chloride ions. This means that in FeCl2, the ratio of iron to chlorine is 1:2 as seen above.

Therefore there is one iron II ion and two chloride ions in each mole of iron II chloride, hence the answer.

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3 years ago

“The chemical formula in the structure of phosphorus is shown below. This represents a(n)....”

den301095 [7]

Answer:

element made up of four (4) similar atoms.

Explanation:

An element is made up of one kind of atom. A compound is made up of 2 or more different kinds of atoms that are chemically together.

5 0

3 years ago

How many grams of sodium are in .500 of a mole

Step2247 [10]

Convert mole to gram by multiplying the molar mass of sodium

0.500mol Na x 22.990g = 11.495g of Na

4 0

3 years ago

The force of gravity pulls down on your house with a total force of 300,000 newtons. The force of gravity pulling down on your h

Nataly [62]

Explanation:

The force of gravity acting on an object is given by :

W = F = mg

Where W is the weight of an object

The force of gravity on house is 300,000 N. The force of gravity pulling down on your house would be exactly twice as much if your house has twice as much as mass because force of gravity is directly depends on mass.

5 0

3 years ago

A student weighs an empty flask and stopper and finds the mass to be 55.844 g. She then adds about 5 mL of an unknown liquid and

Oduvanchick [21]

Answer :

(a) The pressure of the vapor in the flask in atm is, 0.989 atm

(b) The temperature of the vapor in the flask in Kelvin is, 372.7 K

The volume of the flask in liters is, 0.2481 L

(c) The mass of vapor present in the flask was, 0.257 g

(d) The number of moles of vapor present are 0.00802 mole.

(e) The mass of one mole of vapor is 32.0 g/mole

Explanation : Given,

Mass of empty flask and stopper = 55.844 g

Volume of liquid = 5 mL

Temperature = $99.7^oC$

Mass of flask and condensed vapor = 56.101 g

Volume of flask = 248.1 mL

Barometric pressure in the laboratory = 752 mmHg

(a) First we have to determine the pressure of the vapor in the flask in atm.

Pressure of the vapor in the flask = Barometric pressure in the laboratory = 752 mmHg

Conversion used :

$1atm=760mmHg$

or,

$1mmHg=\frac{1}{760}atm$

As, $1mmHg=\frac{1}{760}atm$

So, $752mmHg=\frac{752mmHg}{1mmHg}\times \frac{1}{760}atm=0.989atm$

Thus, the pressure of the vapor in the flask in atm is, 0.989 atm

(b) Now we have to determine the temperature of the vapor in the flask in Kelvin.

Conversion used :

$K=273+^oC$

As, $K=273+^oC$

So, $K=273+99.7=372.7$

Thus, the temperature of the vapor in the flask in Kelvin is, 372.7 K

Now we have to determine the volume of the flask in liters.

Conversion used :

1 L = 1000 mL

or,

1 mL = 0.001 L

As, 1 mL = 0.001 L

So, 248.1 mL = 248.1 × 0.001 L = 0.2481 L

Thus, the volume of the flask in liters is, 0.2481 L

(c) Now we have to determine the mass of vapor that was present in the flask.

Mass of flask and condensed vapor = 56.101 g

Mass of empty flask and stopper = 55.844 g

Mass of vapor in flask = Mass of flask and condensed vapor - Mass of empty flask and stopper

Mass of vapor in flask = 56.101 g - 55.844 g

Mass of vapor in flask = 0.257 g

Thus, the mass of vapor present in the flask was, 0.257 g

(d) Now we have to determine the number of moles of vapor present.

Using ideal gas equation:

PV = nRT

where,

P = Pressure of vapor = 0.989 atm

V = Volume of vapor = 0.2481 L

n = number of moles of vapor = ?

R = Gas constant = 0.0821 L.atm/mol.K

T = Temperature of vapor = 372.7 K

Putting values in above equation, we get:

$(0.989atm)\times 0.2481L=n\times (0.0821L.atm/mol.K)\times 372.7K\\\\n=0.00802mole$

Thus, the number of moles of vapor present are 0.00802 mole.

(e) Now we have to determine the mass of one mole of vapor.

$\text{Mass of one mole of vapor}=\frac{\text{Mass of vapor}}{\text{Moles of vapor}}$

$\text{Mass of one mole of vapor}=\frac{0.257g}{0.00802mole}=32.0g/mole$

Thus, the mass of one mole of vapor is 32.0 g/mole

8 0

3 years ago