CHEMISTRY COLLEGE

Identify the molecule with the strongest intermolecular force.C6H6
OF2
CHCl3
H2O

Answers

Answer 1
Answer:

Answer:

C6H6 has the strongest intermolecular force

i think
Answer 2
Answer:

Answer:

H2O

Explanation:

Because it is a hydrogen bond which is said to be the strongest bond between the H and a N,O, or F combination

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The balanced combustion reaction for C 6 H 6 C6H6 is 2 C 6 H 6 ( l ) + 15 O 2 ( g ) ⟶ 12 CO 2 ( g ) + 6 H 2 O ( l ) + 6542 kJ 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ If 7.300 g C 6 H 6 7.300 g C6H6 is burned and the heat produced from the burning is added to 5691 g 5691 g of water at 21 ∘ 21 ∘ C, what is the final temperature of the water?

Sodium sulfate is slowly added to a solution containing 0.0500 M Ca 2 + ( aq ) and 0.0300 M Ag + ( aq ) . What will be the concentration of Ca 2 + ( aq ) when Ag 2 SO 4 ( s ) begins to precipitate? Solubility-product constants, K sp , can be found in the chempendix.

Answers

Answer : The concentration of [Ca^(2+)] ion is, 0.00371 M

Explanation :

First we have to calculate the concentration of [SO_4^(2-)] ion.

The solubility equilibrium reaction of AgSO_4 will be:

Ag_2SO_4\rightleftharpoons 2Ag^(+)+SO_4^(2-)

The expression for solubility constant for this reaction will be,

K_(sp)=[Ag^(+)]^2[SO_4^(2-)]

K_(sp)=1.20* 10^(-5)

1.20* 10^(-5)=(0.0300)^2* [SO_4^(2-)]

[SO_4^(2-)]=0.0133M

Now we have to calculate the concentration of [Ca^(2+)] ion.

The solubility equilibrium reaction of AgSO_4 will be:

CaSO_4\rightleftharpoons Ca^(2+)+SO_4^(2-)

The expression for solubility constant for this reaction will be,

K_(sp)=[Ca^(2+)][SO_4^(2-)]

K_(sp)=4.93* 10^(-5)

4.93* 10^(-5)=[Ca^(2+)]* (0.0133)  

[Ca^(2+)]=0.00371M

Thus, the concentration of [Ca^(2+)] ion is, 0.00371 M

Final answer:

The concentration of Ca 2+ (aq) will remain constant at 0.0500 M when Ag2SO4 (s) starts to precipitate. This occurs because the precipitation reaction only involves Ag+ (aq), causing its concentration to decrease, while the Ca 2+ (aq) remains unaffected.

Explanation:

To find the concentration of Ca 2+ (aq) when Ag2SO4 (s) begins to precipitate, we start by understanding the concept of the solubility product (Ksp). The Ksp provided in the question (1.6 × 10-¹0) refers to the equilibrium constant for a chemical reaction in which a solid ionic compound dissolves to yield a solution of ions. The precipitation of Ag2SO4 (s) begins when the calculated reaction quotient becomes greater than the solubility product, Ksp. Using this concept, we find that precipitation of Ag2SO4 (s) occurs when the Ag+ (aq) concentration is halved to 1.5 x 10-12 M due to the doubling of the volume when sodium sulfate is added. However, the concentration of Ca 2+ (aq) will remain at 0.0500 M as the Ca 2+ (aq) does not participate in the precipitation reaction.

Learn more about Solubility Product here:

brainly.com/question/35907373

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14) Describe the Cloud Model.

Answers

Electron cloud is an informal term in physics. It is used to describe where electrons are when they go around the nucleus of an atom. The electron cloud model is different from the older Bohr atomic model by Niels Bohr. Bohr talked about electrons orbiting the nucleus.

Wich substances is most likely to form in a precipitation reaction?

Answers

Answer:

A precipitation reaction refers to the formation of an insoluble salt when two solutions containing soluble salts are combined. The insoluble salt that falls out of solution is known as the precipitate, hence the reaction's name.

Explanation:

Glucose, C 6 H 12 O 6 , is used as an energy source by the human body. The overall reaction in the body is described by the equation C 6 H 12 O 6 ( aq ) + 6 O 2 ( g ) ⟶ 6 CO 2 ( g ) + 6 H 2 O ( l ) Calculate the number of grams of oxygen required to convert 58.0 g of glucose to CO 2 and H 2 O . mass of O 2 : 61.76 g Calculate the number of grams of CO 2 produced.

Answers

Answer:

m_(O_2)=61.87gO_2

m_(CO_2)=85.07gCO_2

Explanation:

Hello,

Considering the given reaction's stoichiometry, grams of oxygen result:

m_(O_2)=58.0gC_6H_(12)O_6*(1molC_6H_(12)O_6)/(180gC_6H_(12)O_6)*(6molO_2)/(1molC_6H_(12)O_6)*(32gO_2)/(1molO_2)\nm_(O_2)=61.87gO_2

Moreover, the mass of produced carbon dioxide turns out:

m_(CO_2)=58.0gC_6H_(12)O_6*(1molC_6H_(12)O_6)/(180gC_6H_(12)O_6)*(6molCO_2)/(1molC_6H_(12)O_6)*(44gCO_2)/(1molCO_2)\nm_(O_2)=85.07gCO_2

Best regards.

How many grams of CuSO4 5 H20 are needed to make 1 liter of a 2% (w/v) CuSO4. REPORT TO THE NEAREST 1/10 G.

Answers

Answer:

19.9 grams of CuSO_4.5H_2O will be needed.

Explanation:

Required strength of the solution = 2% (w/v)

This means that 2 gram of solute in 100 ml of solution.

Mass of CuSO_4.5H_2O  = 2 g

Moles of CuSO_4.5H_2O =(2 g)/(249.68 g/mol)=0.008010 mol

Volume of the solution = 100 mL = 0.1 L

Molarity of the solution:

M=(0.008010 mol)/(0.1 L)=0.08010 mol/L

0.08010 moles of CuSO_4.5H_2O are present 1 l of the solution.

Then mass of 0.08010 moles of CuSO_4.H_2O will be:

0.08010 mol × 249.68 g/mol = 19.9993 g≈ 19.9 g

19.9 grams of CuSO_4.5H_2O will be needed.

If a student weighs out 0.744 g Fe ( NO 3 ) 3 ⋅ 9 H 2 O , what is the final concentration of the ∼0.2 M Fe ( NO 3 ) 3 solution that the student makes?

Answers

Answer:

Molar concentration of Fe(NO3)3 . 9H2O = 0.12M

Explanation:

Fe(NO3).9H2O --> Fe(NO3)3 + 9H2O

By stoichiometry,

1 mole of Fe(NO3)3 will be absorb water to form 1 mole of Fe(NO3)3 . 9H2O

Therefore, calculating the mass concentration of Fe(NO3)3;

Molar mass of Fe(NO3)3 = 56 + 3*(14 + (16*3))

= 242 g/mol

Mass concentration of Fe(NO3)3 = molar mass * molar concentration

= 242 * 0.2

= 48.4 g/L

Molar mass of Fe(NO3)3 . 9H2O = 56 + 3*(14 + (16*3)) + 9* ((1*2) + 16)

= 242 + 162 g/mol

= 404g/mol

Concentration of Fe(NO3)3 . 9H2O = mass concentration/molar mass

= 48.4 /404

= 0.12 mol/l

Molar concentration of Fe(NO3)3 . 9H2O = 0.12M
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