Answer: The empirical formula is [tex]CH_2[/tex] and molecular formula is [tex]C_4H_8[/tex]
Explanation:
We are given:
Mass of [tex]CO_2[/tex] = 18.95 g
Mass of [tex]H_2O[/tex]= 7.759 g
Molar mass of carbon dioxide = 44 g/mol
Molar mass of water = 18 g/mol
For calculating the mass of carbon:
In 44g of carbon dioxide, 12 g of carbon is contained.
So, in 18.59 g of carbon dioxide, =[tex]\frac{12}{44}\times 18.59=5.07g[/tex] of carbon will be contained.
For calculating the mass of hydrogen:
In 18g of water, 2 g of hydrogen is contained.
So, in 7.759 g of water, =[tex]\frac{2}{18}\times 7.759=0.862g[/tex] of hydrogen will be contained.
Mass of C = 5.07 g
Mass of H = 0.862 g
Step 1 : convert given masses into moles.
Moles of C =[tex] \frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{5.07g}{12g/mole}=0.422moles[/tex]
Moles of H=[tex]\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.862g}{1g/mole}=0.862moles[/tex]
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For C =[tex]\frac{0.422}{0.422}=1[/tex]
For H =[tex]\frac{0.862}{0.422}=2[/tex]
The ratio of C : H = 1: 2
Hence the empirical formula is [tex]CH_2[/tex].
The empirical weight of [tex]CH_2[/tex] = 1(12)+2(1)= 14 g.
The molecular weight = 56.1 g/mole
Now we have to calculate the molecular formula.
[tex]n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{56.1}{14}=4[/tex]
The molecular formula will be=[tex]4\times CH_2=C_4H_8[/tex]
Hydrogenation (H2/Pd-C) of 3,4-dimethyl-3-hexene (3,4-dimethyl hex-3-ene) would be expected to form A) an enantiomeric pair for both the (E) and (Z) isomers. B) an enantiomeric pair for the (E) isomer and one meso compound for the (Z) isomer. C) one meso compound for the (E) isomer and an enantiomeric pair for the (Z) isomer. D) will not form any stereoisomers since the product is a saturated hydrocarbon. E) None of the above provide a correct response.
Answer:
D) will not form any stereoisomers since the product is a saturated hydrocarbon.
Explanation:
Stereoisomerism, or spatial isomerism,refers to a type of isomerism in which two or more molecules have the same molecular formula and atom to atom connectivity but different three-dimensional orientations of those atoms in space.
Stereoisomerism occurs in alkenes because free rotation about the C=C bond is hindered. Thus, the molecule is "locked" in a particular orientation. In a saturated alkane, there is unrestricted free rotation about the C-C bond hence straight chain alkanes do not have steroisomers.
The product formed is 3,4-dimethyl hexane which is a straight chain saturated alkane. This compound does not exhibit stereoisomerism.
briefly explain formality in solution.
Answer:
Both molarity and formality express concentration as moles of solute per liter of solution. Formality is a substance's total concentration in solution without regard to its specific chemical form. ... The formality of a solution is defined as the number of formula mass of any solute dissolved in 1 litre of solution.
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Answer:
water
Explanation:
because the others are in compounds and can not be considered as products lonely.
why did my dad hasn't come back with the milk for 10 years
Answer:
Milk's heavy
Explanation:
Make a He atom with a mass of 4. How many protons did you put in the nucleus?
Make a Li atom with a mass number of 7. How many electrons did you place in the outermost orbital
(ring)?
Make a N atom with a mass number of 14. How many neutrons are in the nucleus?
Make a B atom with a mass number of 11. How many electrons did you put in the second orbital (ring)?
Answer:
This question appear incomplete
Explanation:
This question appear incomplete. However, let's answer the resulting questions. Firstly, let's define mass number since each of the "problems" refers to mass number. Mass number is the total number of protons and neutrons in the nucleus of an atom. It should also be noted that number of protons in any given neutral atom is the same with the number of electrons of such an atom.
1) Make a He atom with a mass of 4. How many protons did you put in the nucleus?
Answer: Helium (He) atom (having a mass number of 4) has an atomic number of 2. Atomic number is the number of protons and thus 2 protons would be in the nucleus of the Helium atom.
2) Make a Li atom with a mass number of 7. How many electrons did you place in the outermost orbital (ring)?
Answer: Lithium (Li) atom (having a mass number of 7) has an atomic number of 3. Remember that atomic number (number of protons) equals number of electrons in a neutral atom. Thus, lithium atom would have 3 electrons; 2 electrons in it's first shell and 1 electron in it's outermost shell
3) Make a N atom with a mass number of 14. How many neutrons are in the nucleus?
Answer: Nitrogen (N) atom (with a mass number of 14) has an atomic number of 7. Since atomic number is the number of protons and mass number is the number of protons + neutrons. Then, number of neutrons would equal mass number minus atomic number:
number of neutrons = 14 - 7
number of neutrons = 7 neutrons
4) Make a B atom with a mass number of 11. How many electrons did you put in the second orbital (ring)?
Answer: An atom (Boron) with mass number of 11 has an atomic number of 5. Since atomic number eventually equals number of electrons, then Boron has 5 electrons; 2 electrons in it's first shell and 3 electrons in it's second orbital/ring.
Answer:
2 protons in the He nucleus,
1 electron in the outermost,
7 neutrons in the nucleus
3 electrons in the 2nd orbital ring
Explanation:
I just did it on E2020
A mixture of methane and oxygen gases at a total pressure of 727 mm Hg contains methane at a partial pressure of 571 mm Hg. If the gas mixture contains 3.62 grams of methane, how many grams of oxygen are present
Answer: 1.95 g of oxygen is present.
Explanation:
According to Dalton's law, the total pressure is the sum of individual pressures.
[tex]p_{total}=p_{methane}+p_{oxygen}[/tex]
Given : [tex]p_{total}[/tex] =total pressure of gases = 727 mm Hg
[tex]p_{methane}[/tex] = partial pressure of methane = 571 mm Hg
[tex]p_{oxygen}[/tex] = partial pressure of oxygen = ?
[tex]727=571+p_{oxygen}[/tex]
[tex]p_{oxygen}=156mmHg[/tex]
Also [tex]p_{oxygen}=x_{oxygen}\times p_{total}[/tex]
Given : 3.62 g of methane is present
moles of methane = [tex]\frac{\text{Given mass}}{\text {Molar mass}}=\frac{3.62g}{16g/mol}=0.226moles[/tex]
[tex]x_{oxygen}[/tex] = mole fraction of oxygen
=[tex]\frac{\text {moles of oxygen}}{\text {total moles}}=\frac{y}{y+0.226}[/tex]
[tex]156=\frac{y}{y+0.226}\times 727[/tex]
[tex]y=0.061[/tex]
mass of oxygen = [tex]moles\times {\text {Molar mass}}=0.061\times 32=1.95g[/tex]
Thus 1.95 g of oxygen is present.