Chemistry, 11.10.2019 22:40 heroicblad

What is the molecular formula of the compound ch2 with molar mass =168g/mol?

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First, let's find the molar mass of CH₂.

molar mass CH₂= 12.0 + (2 x 1.01)= 14.02 g/mol

Now to determine the molecular formula, we need to find the ratio based in the molar masses.

$\frac{168}{14.02} = 12$

The ratio is 12. so the molecular formula is 12 x CH₂ ----> C₁₂H₂₄

Answer from: PROMASTER

The molecular formula to the given empirical formula is $C_{12}H_{24}$

Explanation:

Empirical formula is defined as the simplest form of the chemical formula that represents the whole number of atoms of each element that are present in the compound. Here, the empirical formula is CH_2

Molecular formula is defined as the chemical formula that represents the actual number of atoms of each element that are present in the compound.

To determine the molecular formula, we first need to determine the valency which is then multiplied by each element to get the molecular formula.

The equation which is used to calculate the valency follows:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

Empirical mass = (12+2)=14g/mol

Molecular mass = 168 g/mol

Putting values in above equation, we get:

$n=\frac{168g/mol}{14g/mol}=12$

Now, multiplying this number to the subscripts of atoms of CH_2 , it gives:

$C_{(1\times 12)}H_{(2\times 12)}=C_{12}H_{24}$

Hence, the molecular formula to the given empirical formula is $C_{12}H_{24}$

Answer from: Quest

You need to divided twenty four by a dozen them by the temperature it is getting cook by

Answer from: Quest

assuming that your periodic table has eighteen columns, you should highlight the four elements in the third column from the left of the table.

explanation

neutral atoms of elements after calcium contain d electrons. the energy of d orbitals of a particular main shell lies between the energy of the s and p orbitals of the next main shell. for example, electrons in the $3d$ have energy higher than those in the $4 s$ orbital while lower than those of the $4 p$ orbital.

by the aufbau principle, electrons fill orbitals one at a time, starting from those of the lowest energy. the $4s$ orbital is therefore filled right after $3p$ orbitals and before $3 d$ orbitals.

potassium has electron configuration $[\text{ar}] 4 s^{1}$ and calcium $[\text{ar}] 4 s^{2}$ . the s orbital of a main shell holds a maximum of two electrons. the next element would thus have the electron configuration $[\text{ar}] 4 s^{2} \; 3d^{1}$ and satisfy the requirements.

a neutral atom of the element contains three electrons on top of the most recent noble gas element. it should thus be placed in the third column of the periodic table. both scandium and yttrium would satisfy the conditions. an aufbau diagram indicates that the 4f orbital is filled before the 5d. however, it appears that exceptions exists for both lanthanum and actinium. neutral atoms of the two d-block elements also demonstrate the $ns^{2} \; (n-1) p^{1}$ and should be highlighted as well.

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