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11Alexandr11 [23.1K]
3 years ago
10

Question 1 (True/False Worth 4 points) (03.06 LC) An instantaneous dipole occurs when a molecule's moving electrons are briefly

more concentrated in one place than another, causing the molecule to become temporarily polarized.
True False

Question 2(Multiple Choice Worth 4 points) (03.06 LC) What type of intermolecular force occurs between all substances?

Covalent bonding
Hydrogen bonding
Ion-dipole force
London dispersion force

Question 3(Multiple Choice Worth 4 points) (03.06 MC) When comparing H2, NH3, O2, and CH4, which of the following statements is correct?

CH4 has the highest boiling point because it experiences dipole-dipole forces.
H2 has the strongest intermolecular forces because it has the lowest mass. NH3 has the highest boiling point because it experiences hydrogen bonding.
O2 has the strongest intermolecular force because it experiences London dispersion forces.

Question 4(Multiple Choice Worth 4 points) (03.06 MC)

The boiling points of diatomic halogens are compared in the table.

Boiling Points of Diatomic Halogens Molecule Boiling Point
F2 −188 °C
Cl2 −34 °C
Br2 59 °C
I2 184 °C
Which of the following statements best explains the trends in boiling points?

The atomic size increases down the group, and this decreases the strength of the intermolecular forces.

The total number of electrons decreases down the group, and this decreases the strength of the intermolecular forces.

The total number of electrons increases down the group, and this increases the strength of the intermolecular forces.

The chances of forming a permanent dipole increase down the group and this increases the strength of the intermolecular forces.

Question 5(Multiple Choice Worth 4 points) (03.06 MC) What is the strongest intermolecular force that occurs between molecules of CO2?

Dipole-dipole
Induced dipoles
Ionic bonding
London dispersion

PLEASE HELP ASAP 30 POINTS...WILL MARK BRAINLIEST
Chemistry
2 answers:
uysha [10]3 years ago
7 0

The answer to question 3 is

C. NH3 has the highest boiling point because it experiences hydrogen bonding.

Pavel [41]3 years ago
3 0
1) True,
when the electrons moving in a molecule or an atom move towards one end of the molecule or atom the other end has a small positive pole at that time and the end where electrons move has a small negative pole. So, a dipole is formed for that instant.

2) London dispersion force,
remember from first part how an instantaneous dipole is formed. When a pole is formed at that instant the molecule in neighborhood can interact with the dipole that was formed. The dipole that was formed has a positive pole and a negative pole. If the neighboring molecule is present near positive pole it’s electrons will get attracted to the positive pole of the dipole. This interaction is called London dispersion force. Since every atom or molecule or ion in the universe has electrons, so there is development of instantaneous dipole in each of them and each one of them has London dispersion force acting on them.

3) one of the option is missing, none of these three is an answer.

4) The total number of electrons increases down the group, and this increases the strength of the intermolecular forces.

5) London dispersion forces which are always present.

London forces are weakest forces, if other forces would have been present then we would have ignored London forces but since no other forces are present, the only choice is London forces.

CO2 is a non polar molecule, it does not have permanent dipole moment. So there are no chances of dipole-dipole, CO2 doesn’t have a positive or negative charge so even not ionic bond.
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How many grams of hydrogen are produced if 30.0 g of zinc reacts?
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<span>0.925 grams if using hydrochloric acid in the reaction. 0.462 grams if using sulfuric acid in the reaction. 0.000 grams if using nitric acid in the reaction. Assuming you're using HCl or a similar acid for this reaction, the equation for the reaction is: Zn + 2 HCl ==> ZnCl2 + H2 So each mole of zinc used, produces 1 mole of hydrogen gas, or 2 moles of hydrogen atoms. So we need to look up the atomic weights of both zinc and hydrogen. Atomic weight zinc = 65.38 Atomic weight hydrogen = 1.00794 Moles zinc = 30.0 g / 65.38 g/mol = 0.458855919 mol Since we produce 2 moles of hydrogen atoms per mole of zinc, multiply by 2 and the atomic weight of hydrogen to get the mass of hydrogen produced. So 0.458855919 * 2 * 1.00794 = 0.92499847 grams. Rounding to 3 significant figures gives 0.925 grams. To show the assumption of the acid used, the balanced equation for sulfuric acid would be Zn2 + H2SO4 ==> Zn(SO4)2 + H2 Which means that for every mole of zinc used, 1 mole of hydrogen gas is generated (half that produced via hydrochloric acid). If nitric acid were used, the reaction is 4Zn + 10HNO3 ==> 4Zn(NO3)2 + N2O + 5H2O Which means that NO hydrogen gas is generated. The only justification for assuming hydrochloric acid is used is that it's a fairly common acid that's easy to obtain. But as shown above with 2 alternative acids, the amount of hydrogen gas generated is very dependent upon the exact chemical reaction occurring and asking "How many grams of hydrogen are produced if 30.0 g of zinc reacts?" is a rather silly question unless you specify EXACTLY what the reaction is.</span>
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<u>Answer:</u> The percent yield of the water is 31.98 %

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}     .....(1)

  • <u>For methane:</u>

Given mass of methane = 6.58 g

Molar mass of methane = 16 g/mol

Putting values in equation 1, we get:

\text{Moles of methane}=\frac{6.58g}{16g/mol}=0.411mol

  • <u>For oxygen gas:</u>

Given mass of oxygen gas = 14.4 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

\text{Moles of oxygen gas}=\frac{14.4g}{32g/mol}=0.45mol

The chemical equation for the combustion of methane is:

CH_4+2O_2\rightarrow CO_2+2H_2O

By Stoichiometry of the reaction:

2 moles of oxygen gas reacts with 1 mole of methane

So, 0.45 moles of oxygen gas will react with = \frac{1}{2}\times 0.45=0.225mol of methane

As, given amount of methane is more than the required amount. So, it is considered as an excess reagent.

Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction

2 moles of oxygen gas produces 2 moles of water

So, 0.45 moles of oxygen gas will produce = \frac{2}{2}\times 0.45=0.45 moles of water

  • Now, calculating the mass of water from equation 1, we get:

Molar mass of water = 18 g/mol

Moles of water = 0.45 moles

Putting values in equation 1, we get:

0.45mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(0.45mol\times 18g/mol)=8.1g

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\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield of water = 2.59 g

Theoretical yield of water = 8.1 g

Putting values in above equation, we get:

\%\text{ yield of water}=\frac{2.59g}{8.1g}\times 100\\\\\% \text{yield of water}=31.98\%

Hence, the percent yield of the water is 31.98 %

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