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3 years ago

How many sigma bonds does CS2 have?

Chemistry

1 answer:

Pie3 years ago

8 0

Answer:

2 sigma bonds

CS2 is called carbon disulphide. The 2 unpaired electrons of each sulphur atom get paired with the 4 unpaired electrons of carbon. But it is a double bond. That is, 2 sigma bonds (sigma s-p , sigma p-p) and 2 pi (πp-p) bonds.

Explanation:

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Which scientist discovered that the atomic number, rather than the atomic weight, is more responsible for the properties of an e

myrzilka [38]

<em>Answer:</em>

The correct option is Moseley who has discovered the atomic number.

<em>Explanation:</em>

In 1913, H. Moseley discovered a new properties of an element atomic number. He observed that elements in the periodic table can be arranged better according to atomic number rather than atomic mass.
The atomic number of any elements is always equal to numbers of electrons in it.

3 0

2 years ago

The diagram shows the process of photosynthesis. Which part represents an autotroph?

Naddik [55]

Answer:

A and B

Explanation:

The Sun's Energy is stored in the chemical bonds that make up food. Some forms of life make their own food. These are the Autotrophs.

Plants are autotrophs, which means they produce their own food.

3 0

1 year ago

Read 2 more answers

Be sure to answer all parts. Consider the reaction N2(g) + 3H2(g) → 2NH3(g)ΔH o rxn = −92.6 kJ/mol If 4.0 moles of N2 react with

Sphinxa [80]

Answer : The work done is, $1.98\times 10^4J$

Explanation :

The given balanced chemical reaction is:

$N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$

When 4 moles of $N_2$ react with 12 moles of $H_2$ then it gives 8 moles of $NH_3$

First we have to calculate the change in moles of gas.

Moles on reactant side = Moles of $N_2$ + Moles of $H_2$

Moles on reactant side = 4 + 12 = 16 moles

Moles on product side = Moles of $NH_3$

Moles on reactant side = 8 moles

Change in moles of gas = 16 - 8 = 8 moles

Now we have to calculate the change in volume of gas.

Using ideal gas equation:

$PV=nRT$

where,

P = Pressure of gas = 1.0 atm

V = Volume of gas = ?

n = number of moles of gas = 8 mole

R = Gas constant = $0.0821L.atm/mol.K$

T = Temperature of gas = $25^oC=273+25=298K$

Putting values in above equation, we get:

$1.0atm\times V=8mole\times (0.0821L.atm/mol.K)\times 298K$

$V=195.7L$

As the number of moles of gas decreased. So, the volume also deceased. Thus, the volume of gas will be, -195.7 L

Now we have to calculate the work done.

Formula used :

$w=-p\Delta V$

where,

w = work done

p = pressure of the gas = 1.0 atm

$\Delta V$ = change in volume = -195.7 L

Now put all the given values in the above formula, we get:

$w=-p\Delta V$

$w=-(1.0atm)\times (-195.7L)$

$w=195.7L.artm=195.7\times 101.3J=19824.41J=1.98\times 10^4J$

conversion used : (1 L.atm = 101.3 J)

Thus, the work done is, $1.98\times 10^4J$

6 0

3 years ago

Are Molar Mass and Molecular Mass the same thing? If they are different, then why are they used interchangeably?

exis [7]

At this point there are two answers: one says that there is no difference, except for the units; the molecular weight (MW) is the mass of one molecule, while a molar mass is the mass of a mole (6.02 x 10 ^ 23) of molecules.

While in certain contexts both statements can be shown to be true, I'm not sure these answers really provide you with the insight you're looking for.

So, we'll look at your question from a different perspective. Take a real example, something simple like water. Water has a nominal MW of 18 (so we'll use nominal precision for simplicity, instead of the 4-places often used for these types of calculations).

The MW of water (formula = H2O) is the weight of one atom of oxygen, which = 16 amu [8-neutrons at 1 amu each plus 8 protons at 1 amu each = 16 amu), plus two atoms of hydrogen, at 1 proton (1 amu) each. Normal everyday hydrogen has no neutrons. So for H2O, we have a total molecular weight of 18 amu.

From the CRC reference book we find that one amu weighs 1.66 x 10 ^--24 grams. Multiplying the two and in keeping with the two units of precision we're working with, one molecule of water has a mass of 29.8 x 10^-24g, or [3.0 x 10 ^ -23 g] per molecule of water.

A Mole is simply Avagadro's number (6.02 x 10 ^ 23) of anything... protons, baseballs, whatever. The term Molar Mass in chemistry refers to the mass of a mole of molecules. So in this case a molar mass of water molecules is Avagadro's number of them, the mass therefore being [6.02 x 10 ^ 23] x 3.0 x 10 ^ -23 g/ molecule] = 18.0 g

Summarizing:

Molecular Weight is the weight given in amu of an atom or molecule. For H2O, the MW is 18 amu or 3.0 x 10 ^ -23 g.

Molar Weight is the weight, usually in grams of 6.02 x 10 ^ 23 measurements which happens to be equal to the MW of the molecule (or atomic wt. of the atom) , and for water is 18.0 g.

So, while MW and molar weight are related, their absolute values are magnitudes apart.

4 0

2 years ago

Read 2 more answers

How many liters of 0.1107 M KCI contain 15.00 g of KCI (FW 74.6 g/mol)? O0.02227 L O 0.5502 L 01661 L O 1.816 L 18.16 L

Greeley [361]

Answer:

1,816 L

Explanation:

Molar concentration or molarity is a way to express the concentration of a chemical in terms of moles of substances per liter of solution.

To obtain the liters of this solution you must convert moles/L to g/L with formula weight (FW), thus:

0,1107 mol of KCl / L × (74,6 g / mol) = 8,258 g of KCl / L.

It means that in one liter you have 8,258 g of KCl. Thus, 15,00 g of KCl are contained in:

15,00 g × (1 L / 8,258 g) = 1,816 L

I hope it helps!

3 0

3 years ago