All categories

3 years ago

Write the condense structural formula of the following compounds.

Chemistry

1 answer:

lozanna [386]3 years ago

3 0

A condensed structural formula is a simple way of representing organic compounds.

The given organic compounds and condensed structural formula is presented below;

The condense structural formula of alkene 2,7 Undecadiene with molecular formula C₁₁H₂₀ is in the image uploaded.
The condense structural formula of 2,8 Nonene with the molecular formula C₉H₁₈ is in the image uploaded.
The condense structural formula of 5 Decyne with the molecular formula C₁₀H₁₈ is in the image uploaded.

Learn more about structural formula here: brainly.com/question/514499

You might be interested in

A gas has a volume of 62.65L at O degrees Celsius and 1 atm. At what temperature in Celsius would the volume of the gas be 78.31

Anastaziya [24]

Answer:

The volume of the gas will be 78.31 L at 1.7 °C.

Explanation:

We can find the temperature of the gas by the ideal gas law equation:

$PV = nRT$

Where:

n: is the number of moles

V: is the volume

T: is the temperature

R: is the gas constant = 0.082 L*atm/(K*mol)

From the initial we can find the number of moles:

$n = \frac{P_{1}V_{1}}{RT_{1}} = \frac{1 atm*62.65 L}{(0.082 L*atm/K*mol)*(0 + 273)K} = 2.80 moles$

Now, we can find the temperature with the final conditions:

$T_{2} = \frac{P_{2}V_{2}}{nR} = \frac{612.0 mmHg*\frac{1 atm}{760 mmHg}*78.31 L}{2.80 moles*0.082 L*atm/(K*mol)} = 274.7 K$

The temperature in Celsius is:

$T_{2} = 274.7 - 273 = 1.7 ^{\circ} C$

Therefore, the volume of the gas will be 78.31 L at 1.7 °C.

I hope it helps you!

8 0

3 years ago

52.1 mL of aqueous 0.255 M Pb(NO3)2 is mixed with 38.5 mL of 0.415 M NaCl. The equation for the precipitate reaction is: Pb(NO3)

Elan Coil [88]

Answer:

0.0585 M

Explanation:

Pb(NO₃)₂ (aq) + 2NaCl (aq) → PbCl₂ (s) + 2NaNO₃ (aq)

First we calculate the inital number of moles of each reagent, using the given volumes and concentrations:

0.255 M Pb(NO₃)₂ * 52.1 mL = 13.3 mmol Pb(NO₃)₂

0.415 M NaCl * 38.5 mL = 16.0 mmol NaCl

Then we calculate how many Pb(NO₃)₂ moles reacted with 16.0 mmoles of NaCl, using the stoichiometric coefficients of the reaction:

16.0 mmol NaCl * $\frac{1mmolPb(NO_3)_2}{2mmolNaCl}$ = 8.00 mmol Pb(NO₃)₂

Now we calculate the remaining number of Pb(NO₃)₂ moles after the reaction:

13.3 mmol - 8.00 mmol = 5.30 mmol Pb(NO₃)₂

Finally we divide the number of moles by the final volume to calculate the concentration:

5.30 mmol / (52.1 mL + 38.5 mL) = 0.0585 M

6 0

3 years ago

What is the molar mass of the following compound: Mg2Ba?

ryzh [129]

Answer:

2(mass no of magnisium)+mass of barium

plug in the values

7 0

3 years ago

An unknown compound contains only C , H , and O . Combustion of 5.90 g of this compound produced 11.8 g CO2 and 4.83 g H2O . Wha

Mamont248 [21]

Answer:

C₂H₄O

Explanation:

In a compound that contains Cabon, hydrogen and oxygen, the combustion produce CO₂ from the carbon, and H₂O from the hydrogens. Using the mass of the products we can solve the moles of Carbon and hydrogen. The empirical formula is the simplest whole-number of atoms present in a molecule.

Moles CO₂ = Moles C:

11.8g CO₂ * (1mol / 44g) = 0.268 moles CO₂ = 0.268 moles C * (12g/mol) =

3.216g C

Moles H₂O = 1/2 moles H:

4.83g H₂O * (1mol / 18g) = 0.268 moles H₂O * (2 mol H / 1 mol H₂O) =

0.537 mol H * (1g/mol) = 0.537g H

Mass O to find moles O:

5.90g Sample - 3.216g C - 0.537g H = 2.147g O * (1mol / 16g) = 0.134 moles O

Ratio of atoms -Dividing in 0.134 moles-:

C = 0.268mol C / 0.134 mol O = 2

H = 0.537mol H / 0.134 mol O = 4

O = 0.134mol O / 0.134 mol O = 1

Empirical formula is:

7 0

3 years ago

Multiple Questions, Brainliest and 98 points to whoever answers all questions correctly

otez555 [7]

Question 1

The average atomic mass of element is 84.66

calculation

Average atomic mass is of an element is the sum of masses of its isotope each multiplied by its natural abundance.

that is.

[(50.50 x 83.75) /100] + [( 30.25 x 84.45)/100] + [(,9.25 x 87.40)/100]

= 42.29 +25.55 +16.82= 84.66

Question 2

fill the table

symbol element protons neutrons Electrons mass No Atomic No

Cs-133 cesium 55 78 55 133 55

Na-23 sodium 11 12 11 23 11

Ne 22 Neon 10 12 1 0 22 10

Au -197 Gold 79 118 79 197 79

Question 3

The moles of tungsten that are in 93.50 grams are 0.509 moles

moles= mass/molar mass

molar mass of tungsten = 183.84 g/mol

moles is therefore= 93.50 g/ 183.84 g/mol= 0.509 moles

question 4

CO2 molecules at STP are 1.547 x10^23 molecules

Step 1: find the moles of CO2

At STP 1 mole of a gas= 22.4 l

? =5.75 L

by cross multiplication

= (5.75 L x 1 mole)/ 22.4 L= 0.257 moles

Step 2: use the Avogadro's constant to calculate the number of molecule

that is 1 moles = 6.02 x10^23 molecules

0.257 moles= ? molecules

by cross multiplication

=(0.257 moles x 6.02 x 10^23) / 1 mole = 1.547 x10^23 molecules

question 5

The number of calcium atoms is 3.82 x10^24 atoms

Step 1: find the moles of calcium

= 253.50 g /40 g/mol= 6.34 moles

Step 2: use the Avogadro's law to calculate the number of atoms.

that is 1 mole= 6.02 x 10^23 atoms

6.34 moles= ? atoms

=6.34 x 6.02 x10^23 = 3.82 x10^24 atoms

Question 6

mass in grams of NiBr2 is 126.97 grams

Step 1: by use of Avogadro's law constant calculate the number of moles

that is 1 mole = 6.02 x 10^23

? = 3.50 x 10^23

by cross multiplication

= (1 mole x 3.50 x10^23) / 6.02 x10^23 =0.581 moles

step 2: calculate the mass

mass =moles x molar mass

= 0.581 moles x218.53 g/mol = 126.97 grams

Bonus question

The molecules of water= 1.00 x10^26 molecules

calculation

convert liters into ml

= 3 x 1000 = 3000 ml

find the mass of water

= density x volume

=3000 x0.998 2994 grams

find the moles of water=mass/molar mass

= 2994 g/ 18 g/mol= 166.33 moles

Use Avogadro's constant to calculate the molecules of water

that is 1 mole= 6.02 x10^23 molecules

166.33 moles= ? molecules

= (166.33 moles x6.02 x10^23 molecules) / 1 mole = 1.00 x10^26 molecules

3 0

3 years ago

Read 2 more answers