In ionic bonds, valence electrons are

Calculate the mass of Cr(ClO2)2 that contains 5.57 × 10<br> ^22 chlorine atoms.

Anna007 [38]

Answer:

Explanation:

Your strategy here will be to

use the chemical formula of carbon dioxide to find the number of molecules of

CO

2

that would contain that many atoms of oxygen

use Avogadro's constant to convert the number of molecules to moles of carbon dioxide

use the molar mass of carbon dioxide to convert the moles to grams

So, you know that one molecule of carbon dioxide contains

one atom of carbon,

1

×

C

two atoms of oxygen,

2

×

O

This means that the given number of atoms of oxygen would correspond to

4.8

⋅

10

22

atoms O

⋅

1 molecule CO

2

atoms O

=

2.4

⋅

10

22

molecules CO

2

Now, one mole of any molecular substance contains exactly

6.022

⋅

10

22

molecules of that substance -- this is known as Avogadro's constant.

In your case, the sample of carbon dioxide molecules contains

2.4

⋅

10

22

molecules CO

2

⋅

1 mole CO

2

6.022

⋅

10

23

molecules CO

2

=

0.03985 moles CO

2

Finally, carbon dioxide has a molar mass of

44.01 g mol

−

1

, which means that your sample will have a mass of

0.03985

moles CO

2

⋅

44.01 g

1

mole CO

2

=

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

∣

a

1.8 g

a

∣

−−−−−−−−−

The answer is rounded to two sig figs, the number of sig figs you have for the number of atoms of oxygen present in the sample.

3 0

2 years ago

Write balanced chemical equations for the sequence of reactions that oxalic acid can undergo when it's dissolved in water.

Mashcka [7]

Answer and Explanation:

The balanced chemical equations are as follows:

The chemical formula of oxalic is $H_2C_2O_4$

In the case when oxalic acts reacted with the water so here the oxalic acid eliminates one proton that leads to the development of mono acids

After that, the second step derives that when oxalic acid is in aqueous solution eliminates other proton so it represent the polyprotic acid

Now the chemical equations are as follows:

Elimination of one proton

$H_2C_2O_4(aq)+H_2O(l) \rightarrow H_2C_2O_4^-(aq) + H_3O^+(aq)$

Now the elimination of other proton

$HC_2O_4^-(aq)+H_2O(l) \rightarrow C_2O_4^2^-(aq) + H_3O^+(aq)$

7 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

Which family in the periodic table has elements that are silvery and lustrous?

IrinaVladis [17]

The correct answer is A. Alkali metals.
I hope this helped

6 0

3 years ago

Read 2 more answers

A cylinder containing carbon dioxide of volume 20 L at 2.0 atm was connected to another cylinder of certain volume at constant t

den301095 [7]

Answer:

The volume of the second cylinder is 80 liters

Explanation:

We use the Boyle-Mariotte formula, according to which the pressure and volume of a gas are inversely related, keeping the temperature constant: P1 x V1 = P2xV2. We convert the pressure in mmHg to atm:

760 mmHg-----1 atm

380mmHg------x= (380mmHgx1atm)/760mmHg=0,5 atm

P1xV1=P2xV2

2 atmx20 L= 0,5atm x V2 V2=(2 atmx20 L)/0,5atm=80L

8 0

3 years ago