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cestrela7 [59]
3 years ago
12

From this list, choose all of the ionic compounds. Check all that apply. View Available Hint(s) Check all that apply. POCl3 KOCH

2CH3 CH3OH SOCl2 CH3CH2CO2Na NaOH CH2
Chemistry
1 answer:
Alik [6]3 years ago
4 0

Answer: KOCH_2CH_3, CH_3CH_2COONa, NaOH are all ionic compounds.

Explanation:

It is known that ionic compounds are the compounds in which one atom transfer its valence electrons to another atom. Hence, during this transfer partial opposite charges tend to develop on the combing atoms due to which strong force of attraction exists between the atoms.

An ionic bond is always formed between a metal and a non-metal.

For example, KOCH_2CH_3, CH_3CH_2COONa, NaOH are all ionic compounds.

On the other hand, a compound formed due to sharing of electrons between the combining atoms is known as a covalent compound. Generally, a non-metal with same or different non-metal tends to form a covalent bond.

For example, POCl_{3}, SOCl_{2} etc are all covalent compounds.

Thus, we can conclude that KOCH_2CH_3, [tex]CH_3CH_2COONa, NaOH are all ionic compounds.

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If 9.9L of helium are in a tire at 303k,how many liters will be present at 403k if the pressure is held constant.
Slav-nsk [51]

Answer:

Final volume, V2 = 13.18 Liters

Explanation:

<u>Given the following data;</u>

Initial volume = 9.9 L

Initial temperature = 303 K

Final temperature = 403 K

To find the final volume, we would use Charles law;

Charles states that when the pressure of an ideal gas is kept constant, the volume of the gas is directly proportional to the absolute temperature of the gas.

Mathematically, Charles' law is given by the formula;

VT = K

\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}

Where;

  • V1 and V2 represents the initial and final volumes respectively.
  • T1 and T2 represents the initial and final temperatures respectively.

\frac{V1}{T1} = \frac{V2}{T2}

Making V2 as the subject formula, we have;

V_{2}= \frac{V1}{T1} * T_{2}

V_{2}= \frac{9.9}{303} * 403

V_{2}= 0.0327 * 403

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8 0
3 years ago
The density of the hydrocarbon in part (a) is 2.0 g l-1 at 50°c and 0.948atm. (i) calculate the molar mass of the hydrocarbon. (
Vedmedyk [2.9K]

1. Answer;

=56 g/mol

Explanation and solution;

PV = nRT

nRT= mass/molar mass (RT)

molar mass = (mass/V ) × (RT/P)

                   = Density × (RT/P)

Molar mass = 2.0 g/L × (0.0821 × 323 K)/0.948 atm

Molar mass = 56 g/mol


2. Answer;

Molecular mass is C4H8

Explanation;

Empirical mass × n = molar mass

Empirical mass for CH2 = 14 g/mol

Therefore;

56 g/mol = 14 g/mol × n

   n = 4

The molecular formula= 4(CH2)

    = C4H8


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