What bond distance is expected to be longest?1. A carbon-carbon bond with a bond order of 2
2. A carbon-carbon bond with a bond order of 3
3. A carbon-carbon bond with a bond order of O
4. carbon-carbon bond with a bond order of 1

Answers

Answer 1

Answer:

Answer:

Bond length of C=C is largest(134 pm) because both the carbon atoms have same electronegativity. In case of C=O. and C=N carbon is bonded to highly electronegative atoms so bond length is shoreter as compared to C=C

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Ne ( g ) effuses at a rate that is ______ times that of Cl 2 ( g ) under the same conditions.

Answers

Answer: 1.88times as that of Cl2

Explanation:

According to Graham law of effusion , the rate of effusion is inversely proportional to the square root of the molar mass

Rate= 1/√M

R1/R2 =√M2/M1

Let the rate of diffusion of Ne= R1

And rate of diffusion of Cl2 = R2

M1 ,molar mass of Ne= 20g/mol

M2,molar mass of Cl2 =71g/mol

R1/R2 = √ (71/20)

R1/R2 = 1.88

R1= 1.88R2

Therefore the Ne effuses at rate that is 1.88times than that of Cl2 at the same condition.

A particular refrigerant cools by evaporating liquefied CCl 2F 2. How many kg of the liquid must be evaporated to freeze a tray of water to ice (at zero degrees C)? The tray contains 525 grams water. Molar heat of fusion of ice = 6.01 kJ/mol. Molar heat of vaporization of CCl 2F 2 = 17.4 kJ/mole

Answers

Answer : The mass of $CCl_2F_2$ evaporated must be, 1.217 kg

Explanation :

First we have to calculate the moles of water.

$\text{Moles of water}=\frac{\text{Mass of water}}{\text{Molar mass of water}}$

Molar mass of water = 18 g/mol

$\text{Moles of water}=(525g)/(18g/mol)=29.17mol$

Now we have to calculate the heat released.

Heat released = Moles of water × Molar heat of fusion of ice

Heat released = 29.17 mol × 6.01 kJ/mol

Heat released = 175.3 kJ

Now we have to calculate the moles of $CCl_2F_2$

Heat = Moles of $CCl_2F_2$ × Molar heat of vaporization of $CCl_2F_2$

175.3 kJ = Moles of $CCl_2F_2$ × 17.4 kJ/mol

Moles of $CCl_2F_2$ = 10.07 mol

Now we have to calculate the mass of $CCl_2F_2$

$\text{Mass of }CCl_2F_2=\text{Moles of }CCl_2F_2* \text{Molar mass of }CCl_2F_2$

Molar mass of $CCl_2F_2$ = 120.9 g/mol

$\text{Mass of }CCl_2F_2=10.07mol* 120.9g/mol=1217.463g=1.217kg$

Thus, the mass of $CCl_2F_2$ evaporated must be, 1.217 kg

PLEASE HELP ASAP!!1. what is the pOH of a solution if the pH is 2.23?

A. pOH=13
B. pOH=11.77
C. pOH=8.52
D. pOH=10.52

2. what is the pOH of a solution if the pH is 2.23

A. pOH=1
B. pOH=12
C. pOH=8
D. pOH=9

3. Given a solution of perchloric acid has a concentration of .023M, what is the pH and pOH

A. pH=2.3 and pOH=11.97
B. pH=1.64 and pOH= 12.36
C. pH=4.5 and pOH=9.95

Answers

1) POH=14-2.23=11.77
2)B
3)HClO4=H+ +clo4—
C(H+)=0.023 M
pH=-log[H+]=1.63
POH=14-1.63=12.37

Final answer:

The pH and pOH for a solution are related through the equation pH + pOH = 14. The pOH for solutions with a pH of 2.23 is 11.77, and in a solution of perchloric acid with a concentration of .023M, the pH is 1.64 and pOH is 12.36.

Explanation:

The concept of pOH and pH are related through the equation pH + pOH = 14 at 25 °C. If you have the value of one, you can easily find the other. For your first two questions, the pH of solution is given as 2.23. Therefore, the pOH would be 14 - 2.23 = 11.77. Your answer to both questions 1 and 2 is B. pOH=11.77.

For question 3, the perchloric acid has a concentration of .023M. To find the pH, we calculate -log[H3O+], which gives about 1.64. Therefore, the pOH would be 14 - 1.64 = 12.36. Your answer to question 3 is B. pH=1.64 and pOH=12.36.

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Write for empiricalformula
Fe2+, cr4+, cl-, O2-

Answers

Answer:

{eq}Fe^{2+} {/eq} and {eq}I^- {/eq} forms {eq}FeI_2 {/eq}

{eq}Fe^{2+} {/eq} and {eq}S^{2-} {/eq} forms {eq}FeS {/eq}

{eq}Cr^{4+} {/eq} and...

Explanation:

Empirical formula:

The empirical formula gives the simple ratio of the different types of atoms in a compound. It is different from the molecular formula, which gives the exact number of each type of atom in a compound.

Final answer:

In basic chemistry, an empirical formula represents the simplest ratio of atoms in a compound. For example, the empirical formula for a compound formed by Fe2+ (Iron II) and O2- (Oxide) would be FeO. In this question, a compound composed of all these ions (Fe2+, Cr4+, Cl-, O2-) is unusual and there's insufficient information to determine a reasonable structure.

Explanation:

The question is asking for an empirical formula, which is a formula that gives the simplest whole number ratio of atoms of each element in a compound. The formula you're asked to provide involves the ions Fe2+ (Iron II), Cr4+ (Chromium IV), Cl- (Chloride), and O2- (Oxide).

Creating an empirical formula is a matter of balancing out the charges in order to get a neutral compound. For instance, if you wanted to combine Fe2+ and O2-, the empirical formula would be FeO because one Fe2+ ion would balance out one O2- ion to make an electrically neutral compound.

It's important to remember that the charge value of the ion helps you determine the necessary ratio to achieve neutrality. In essence, we need the amount of positive charge to equal the amount of negative charge in the empirical formula.

For a compound involving all these ions, unfortunately, it's not common or reasonable to have a compound with four different ions. Iron, chromium, and oxygen are transition metals that could form complex ions, but we do not have enough information in this question to determine the structure.

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NEED HELP!
C=46.67%, H=4.48%, N=31.10%, O=17.76%.
The molecular weight is 180.16g/mol.

Answers

Answer:

$C_7H_8N_4O_2$

Explanation:

Hello!

In this case, since the determination of an empirical formula is covered by first computing the moles of each atom as shown below:

$n_C=(46.47g)/(12g/mol)=3.9mol\n\n n_H=(4.48g)/(1g/mol) =4.5mol\n\nn_N=(31.10g)/(14g/mol) =2.2mol\n\nn_O=(17.76g)/(16g/mol) =1.1mol$

Now, we divide each moles by the fewest moles (those of oxygen), to obtain the subscripts in the empirical formula:

$C:(3.9)/(1.1)=3.5 \n\nH:(4.5)/(1.1)=4 \n\nN:(2.2)/(1.1) =2\n\nO:(1.1)/(1.1) =1$

Thus, the empirical formula, taken to the nearest whole subscript is:

$C_7H_8N_4O_2$

Whose molar mass is 180.16, therefore the empirical formula is the same to the molecular one.

Best regards!

What would the initial pH of a acetate/acetic acid buffer system (pKa = 4.75) if the concentration of acetate is 1.36 × 10-2 molar and the concentration of acetic acid is 1.64 × 10-1?A.
5.83
B.
3.67
C.
2.08
D.
1.66