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2 years ago

Arranges the following molecules in order of increasing dipole moment: H2O, H2S, H2Te, H2Se.

Chemistry

1 answer:

erastova [34]2 years ago

7 0

Explanation:

Dipole moment is defined as the measurement of the separation of two opposite electrical charges.

$H_{2}O$ is a bent shaped molecule with a dipole moment of 1.87.

$H_{2}S$ is also a bent shaped molecule with a dipole moment of 1.10.

$H_{2}Te$ is a also a bent shaped molecule and has a negligible dipole moment.

$H_{2}Se$ has a dipole moment of 0.29.

Therefore, given molecules are arranged according to their increasing dipole moment as follows.

$H_{2}Te$ < $H_{2}Se$ < $H_{2}S$ < $H_{2}O$

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An unknown compound with a molar mass of 155.06 g/mol consists of 46.47% c, 7.80% h, and 45.72% cl. find the molecular formula f

Contact [7]

Answer:- Molecular formula of the compound is $C_6H_1_2Cl_2$ .

Solution:- From given information:

C = 46.47%

H = 7.80%

Cl = 45.72%

First of all we find out the empirical formula from given percentages. We divide the given percentages by their respective atomic masses to calculate the moles:

$C=\frac{46.47}{12.01}$ = 3.87

$H=\frac{7.80}{1.01}$ = 7.72

$Cl=\frac{45.72}{35.45}$ = 1.29

Now, we divide the moles of each by the least one of them. Least one is Cl as it's moles are least as compared to the moles of C and H. So, let's divide the moles of each by 1.29.

$C=\frac{3.87}{1.29}$ = 3

$H=\frac{7.72}{1.29}$ = 6

$Cl=\frac{1.29}{1.29}$ = 1

So, the empirical formula of the compound is $C_3H_6Cl$ .

Empirical formula mass = 3(12.01) + 6(1.01) + 1(35.45)

= 36.03 + 6.06 + 35.45

= 77.54

To calculate the number of formula units we divide molar mass by empirical formula mass.

number of empirical formula units = $\frac{155.06}{77.54}$

= 2

So, the molecular formula would be two times of empirical formula that is, $C_6H_1_2Cl_2$ .

4 0

2 years ago

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A scientist has isolated a fatty acid that has 26 carbons bonded together. most of the carbon atoms in the chain are connected b

Tasya [4]

This is a monounsaturated fatty acid .
Saturated fatty acids are those where all the C atoms are bonded by single bonds.
When they are bonded by single bonds, each C has the maximum amount of H atoms it can bond to. It’s then saturated with H atoms.
When there are fatty acids with double bonds, then they are called unsaturated bonds as they don’t have the maximum number of H atoms.
The fatty acid in the question all the C atoms are bonded by single bonds except for one double bond , therefore it’s monounsaturated fatty acid

7 0

2 years ago

One of the most recognizable corrosion reactions is the rusting of iron. rust is caused by iron reacting with oxygen gas in the

zloy xaker [14]

Answer: $Fe(s) + 6H_2O(l) + 3O_2(g) -> 4Fe(OH)_3(s)$

Explanation:

The Chemical equation for the formation of rust is:

Iron + Water + Oxygen ----> Rust

4 Fe(s) + 6 H2O(l) + 3 O2(g) → 4 Fe(OH)3(s)

The Iron Hydroxide However dehydrates to produce Fe2O3 * nH2O

3 0

2 years ago

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Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.a. 0.0200 mol sodium p

JulsSmile [24]

Answer:

For a: The concentration of $Na^+\text{ and }PO_4^{3-}$ ions in the solution are 6 M and 2 M respectively.

For b: The concentration of $Ba^{2+}\text{ and }NO_3^{-}$ ions in the solution are 0.5 M and 1.0 M respectively.

For c: The concentration of $K^{+}\text{ and }Cl^{-}$ ions in the solution are 0.051 M and 0.051 M respectively.

For d: The concentration of $NH_4^{+}\text{ and }SO_4^{2-}$ ions in the solution are 1.34 M and 0.67 M respectively.

Explanation:

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}$ ......(1)

Or,

$\text{Molarity of the solution}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}$ ...(2)

For the given options:

For a:

The chemical formula of sodium phosphate is $Na_3PO_4$

Moles of sodium phosphate = 0.0200 moles

Volume of solution = 10.0 mL

Putting values in equation 1, we get:

$\text{Molarity of the sodium phosphate}=\frac{0.0200\times 1000}{10.0}=2M$

1 mole of sodium phosphate produces 3 moles of $Na^+$ ions and 1 mole of $PO_4^{3-}$ ions

So, concentration of $Na^+\text{ ions}=(3\times 2)=6M$

Concentration of $PO_4^{3-}\text{ ions}=(1\times 2)=2M$

Hence, the concentration of $Na^+\text{ and }PO_4^{3-}$ ions in the solution are 6 M and 2 M respectively.

For b:

The chemical formula of barium nitrate is $Ba(NO_3)_2$

Moles of barium nitrate = 0.300 moles

Volume of solution = 600.0 mL

Putting values in equation 1, we get:

$\text{Molarity of the barium nitrate}=\frac{0.300\times 1000}{600.0}=0.5M$

1 mole of barium nitrate produces 1 mole of $Ba^{2+}$ ions and 2 mole of $NO_3^{-}$ ions

So, concentration of $Ba^{2+}\text{ ions}=(1\times 0.5)=0.5M$

Concentration of $NO_3^{-}\text{ ions}=(2\times 0.5)=1M$

Hence, the concentration of $Ba^{2+}\text{ and }NO_3^{-}$ ions in the solution are 0.5 M and 1.0 M respectively.

For c:

The chemical formula of potassium chloride is KCl

Given mass of potassium chloride = 1.00 g

Molar mass of potassium chloride = 39 g/mol

Volume of solution = 0.500 L

Putting values in equation 1, we get:

$\text{Molarity of the potassium chloride}=\frac{1.00}{39\times 0.500}=0.051M$

1 mole of potassium chloride produces 1 mole of $K^{+}$ ions and 1 mole of $Cl^{-}$ ions

So, concentration of $K^{+}\text{ ions}=(1\times 0.051)=0.051M$

Concentration of $Cl^{-}\text{ ions}=(1\times 0.051)=0.051M$

Hence, the concentration of $K^{+}\text{ and }Cl^{-}$ ions in the solution are 0.051 M and 0.051 M respectively.

For d:

The chemical formula of ammonium sulfate is $(NH_4)_2SO_4$

Given mass of ammonium sulfate = 132 g

Molar mass of ammonium sulfate = 132 g/mol

Volume of solution = 1.50 L

Putting values in equation 1, we get:

$\text{Molarity of the ammonium sulfate}=\frac{132}{132\times 1.50}=0.67M$

1 mole of ammonium sulfate produces 2 moles of $NH_4^{+}$ ions and 1 mole of $SO_4^{2-}$ ions

So, concentration of $NH_4^{+}\text{ ions}=(2\times 0.67)=1.34M$

Concentration of $SO_4^{2-}\text{ ions}=(1\times 0.67)=0.67M$

Hence, the concentration of $NH_4^{+}\text{ and }SO_4^{2-}$ ions in the solution are 1.34 M and 0.67 M respectively.

4 0

2 years ago

Calculate the mass of hydrazine (N2H4) that contains a billion (1.000 x 10^9) hydrogen atoms.

Lunna [17]

Answer:

1.3285 × 10⁻¹⁴ g of hydrazine

Explanation:

if 32 g of hydrizine (1 mole) contains 4 × 6.022 × 10²³ hydrogen atoms

then X g of hydrizine contains 1 × 10⁹ hydrogen atoms

X = (32 × 1 × 10⁹) / (4 × 6.022 × 10²³)

X = 1.3285 × 10⁻¹⁴ g of hydrazine

3 0

2 years ago

Read 2 more answers