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alexira [117]
2 years ago
7

In table below, there are descriptions of an experiment on samples of three different chemical compounds. Decide whether the com

pound is ionic or molecular, if you can. If there is not enough information to decide, choose can't decide in the third column.
Compound Description Ionic or Molecular
1 Compound 1 is a light gray solid made of overlapping
hexagonal crystals. When heated gently it starts to soften
and develop an unpleasant smell about 50 °C. above
room temperature.
2 Compound 2 is a deep red solid with a noticeable
unpleasant smell. It dissolves slightly in water, and
a solution of 2 g in 100 mL of water doesn't change the
electrical conductivity of the water.
3 Compound 3 is a clear liquid with a strong smell. If
heated gently it boils at 115. °C.
Chemistry
1 answer:
Ulleksa [173]2 years ago
8 0

Answer:

1. molecular

2. molecular

3. molecular

Explanation:

Molecular compounds typically exhibit covalent compound characteristics. They are pure substances formed when atoms are linked together by sharing electrons while ionic compounds are formed due to the transfer of electrons. Molecular substances tend to melt at moderately warm temperatures (i.e. 50° C) and it is overlapping as seen in compound 1, which makes it to be molecular in nature.

Molecular compounds are not affected by conductivity, hence they are electrically neutral.

Molecular compounds have a strong smell and have freezing and boiling point at accessible temperatures. A clear liquid at room temperature which has a fruity strong smell can be an organic compound. These organic compounds made up of covalent bonds and are molecular in nature.

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Svetach [21]

Answer:

is

Explanation:

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3 0
3 years ago
A sample of He gas (3.0 L) at 5.6 atm and 25°C was combined with 4.5 L of Ne gas at 3.6 atm and 25°C at constant temperature in
LenKa [72]

Answer:

P=3.7atm

Explanation:

Hello,

In this case, it is possible to determine the pressures of both helium and neon as shown below:

n_{He}=\frac{P_{He}V_{He}}{RT}=\frac{5.6atm*3.0L}{0.082\frac{atm*L}{mol*K}*298.15K} =0.688molHe\\\\n_{Ne}=\frac{P_{Ne}V_{Ne}}{RT}=\frac{3.6atm*4.5L}{0.082\frac{atm*L}{mol*K}*298.15K}=0.663molNe

Now, one considers the total moles (addition between both neon's and helium's moles) and the total volume to compute the final pressure as shown below:

P=\frac{n_TRT}{V_T} =\frac{(0.688+0.663)mol*0.082\frac{atm*L}{mol*K}*298.15K}{9.0L}=3.7atm

Best regards.

8 0
2 years ago
A 25-mL solution of H2SO4 is completely neutralized by 18 mL of 1.0M NaOH. What is the concentration of the H2SO4?
Charra [1.4K]
There are several information's already given in the question. Based on the information's provided, the answer can be easily deduced.
V1 = 25 ml
     = 25/1000 liter
     = 0.025 liter
V2 = 18 ml
      = 18/1000 liter
      = 0.018 liter
M2 = 1.0 M
M1 = ?
Then
M1V1 = M2V2
M1 = M2V2/V1
      = (1 * 0.018)/0.025
      = 0.72 M
From the above deduction, it can be easily concluded that the correct option among all the options that are given in the question is the first option or option "A". I hope that this is the answer that has actually come to your help.
5 0
3 years ago
Read 2 more answers
What term is best described as the rate of a chemical reaction at any instant in time?
Fantom [35]

Answer:

instantaneous rate would be the term.

5 0
1 year ago
How many grams of oxygen gas occupy 12.3 L of space at 109.4 kPa and 15.4oC?
I am Lyosha [343]

17.93 grams of oxygen gas occupy 12.3L of space at 109.4 kPa and 15.4°C. Details about how to calculate mass can be found below.

<h3>How to calculate mass?</h3>

The mass of a given gas can be calculated by multiplying the number of moles of the substance by its molar mass.

However, the number of moles of the gas must be calculated first as follows:

PV = nRT

Where;

  • P = pressure = 1.0796941atm
  • V = volume = 12.3L
  • n = number of moles
  • T = temperature = 288.4K
  • R = gas law constant = 0.0821 Latm/molK

1.079 × 12.3 = n × 0.0821 × 288.4

13.27 = 23.68n

n = 13.27/23.68

n = 0.56mol

Mass = 0.56 × 32

mass of oxygen gas = 17.93g

Therefore, 17.93 grams of oxygen gas occupy 12.3L of space at 109.4 kPa and 15.4°C.

Learn more about mass at: brainly.com/question/19694949

3 0
1 year ago
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