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3 years ago

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How many lone pairs does CO2 have? Does it have Single bonds or Double bonds? Does it obey the octet rule?

1 answer:

Aleks04 [339]3 years ago

3 0

The molecule CO2 have 2 lone pairs located in the oxygen atoms. It has two double bonds also connecting carbon atom to the two oxygen atoms. It does obey the octet rule so the atoms need 8 electrons in each of them that is why electrons are shared.

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Each step in the following process has a yield of 90.0 %. CH 4 + 4 Cl 2 ⟶ CCl 4 + 4 HCl CCl 4 + 2 HF ⟶ CCl 2 F 2 + 2 HCl The CCl

Rainbow [258]

Answer:

4.86 moles of HCl

Explanation:

1. First write the balanced chemical equations involved in the process:

$CH_{4}+_4Cl_{2}=CCl_{4}+_4HCl$

$CCl_{4}+_2HF=CCl_{2}+F_{2}+_2HCl$

2. Calculate what amount of $CCl_{4}$ is formed in the first reaction.

$3.00molesCH_{4}*\frac{1molCCl_{4}}{1molCH_{4}}=3.00molesCCl_{4}$

As the yield of each reaction is 90.0%, the amount of $CCl_{4}$ produced is the following:

$3.00molesCCl_{4}*0.90=2.7molesCCl_{4}$

3. Calculate the amount of HCl produced.

$2.7molesCCl_{4}*\frac{2molHCl}{1molCCl_{4}}=5.4molesHCl$

The total amount of HCl produced with a 90.0% yield is:

$5.4molesHCl*0.90=4.86molesHCl$

4 0

3 years ago

A sample of a gas is occupying a 1500 ml container at a pressure of 3.4 atm and a temperature of 25 oc. if the temperature is in

Salsk061 [2.6K]

The new pressure will be 7.65 atm

<h3>General gas law</h3>

The problem is solved using the general gas equation:

P1V1/T1 = P2V2/T2

In this case, P1 = 3.4 atm, V1 = 1500 mL, T1 = 25 $^O C$ , V2 = 2000 mL, and T2 = 75 $^O C$

What we are looking for is P2.

Thus, P2 = P1V1T2/T1V2

= 3.4 x 1500 x 75/25 x 2000 = 382500/50000 = 7.65 atm

More on general gas laws can be found here: brainly.com/question/2542293

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7 0

2 years ago

A 850.0 mL cylinder containing B2H6 at a pressure of 0.900 atm is connected by a valve to 1000 mL cylinder containing C6H6 at 60

8_murik_8 [283]

Answer:

The partial pressure of $C_6H_6$ when the valve is opened is 328.6 Torr.

Explanation:

Initial pressure of the $C_6H_6=P_1=608.0 Torr$

Initial volume of the $C_6H_6=V_1=1000 mL$

After opening the valve :

Final pressure or partail pressure of the $C_6H_6=P_2$

Final volume of the $C_6H_6=V_2=1000 mL+850.0 mL=1850.0 mL$

$P_1V_1=P_2V_2$ ( Boyle's law)

$P_2=\frac{608.0 Torr \times 1000 mL}{1850.0 mL}=328.6 Torr$

The partial pressure of $C_6H_6$ when the valve is opened is 328.6 Torr.

4 0

3 years ago

Enter your answer in the box provided. How many grams of helium must be added to a balloon containing 6.24 g helium gas to doubl

Archy [21]

Answer : The mass of helium gas added must be 12.48 grams.

Explanation : Given,

Mass of helium (He) gas = 6.24 g

Molar mass of helium = 4 g/mole

First we have to calculate the moles of helium gas.

$\text{Moles of }He=\frac{\text{Mass of }He}{\text{Molar mass of }He}=\frac{6.24g}{4g/mole}=1.56moles$

Now we have to calculate the moles of helium gas at doubled volume.

According to the Avogadro's law, the volume of gas is directly proportional to the number of moles of gas at same pressure and temperature. That means,

$V\propto n$

or,

$\frac{V_1}{V_2}=\frac{n_1}{n_2}$

where,

$V_1$ = initial volume of gas = V

$V_2$ = final volume of gas = 2V

$n_1$ = initial moles of gas = 1.56 mole

$n_2$ = final moles of gas = ?

Now we put all the given values in this formula, we get

$\frac{V}{2V}=\frac{1.56mole}{n_2}$

$n_2=3.12mole$

Now we have to calculate the mass of helium gas at doubled volume.

$\text{Mass of }He=\text{Moles of }He\times \text{Molar mass of }He$

$\text{Mass of }He=3.12mole\times 4g/mole=12.48g$

Therefore, the mass of helium gas added must be 12.48 grams.

4 0

3 years ago

3. Meteorologists refer to the water vapor in the atmosphere as

Oduvanchick [21]

A. Humidity

I hope this helped!

8 0

3 years ago

Read 2 more answers