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Ymorist [56]
2 years ago
7

Help ASAP! Answer the question and be made the Brainliest

Chemistry
1 answer:
bekas [8.4K]2 years ago
5 0
1. A
2. B
3. B
4. D
5. C
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Which of the following are properties of compounds formed by ionic bonding? Hint: Select the best three answers.
marysya [2.9K]

Answer:

the correct answers are:

B

E

G

4 0
2 years ago
____is not a resource that can be used to help meet our energy needs
Bezzdna [24]
I believe the answer to this is A. 
7 0
3 years ago
Select all that apply.
alexgriva [62]

Hi!


<u>The correct options would be: </u>

is an electron

is emitted from nucleus

has a -1 charge


Explanation:

A beta particle is a result of a neutron (a neutral particle) changing into two particles of opposite charges - a high energy electron (with a negative charge -1) and a positron (with a positive charge +1). Neutrons are present in the nucleus of an atom, and thus the beta particles are said to be emitted from the nucleus. They do have a charge, not zero, but it is not +2 and can only be either -1 or +1. This form of radiation is not electromagnetic energy because beta particles are massless, and do not travel at the speed of light (both being characteristics of electromagnetic radiation). Beta particles are not pure forms of energy.


Hope this helps.

6 0
2 years ago
A student is instructed to make 1 L of a 2.0 M solution of CaCl2 using dry salt. How should he do this?
Pachacha [2.7K]
<span>The student should follow following steps to make 1 L of </span>2.0 M CaCl₂.<span>
<span>
1. First he should calculate the number of moles of 2.0 M CaCl</span></span>₂ in 1 L solution.<span>

</span>Molarity of the solution = 2.0 M<span>
Volume of solution which should be prepared = 1 L

Molarity = number of moles / volume of the solution

Hence, number of moles in 1 L = 2 mol

2. Find out the mass of dry CaCl</span>₂ in 2 moles.<span>

moles = mass / molar mass

Moles of CaCl₂ = 2 mol</span><span>
Molar mass of CaCl₂ = </span><span>110.98 g/mol

Hence, mass of CaCl</span>₂ = 2 mol x <span>110.98 g/mol
                                     = 221.96 g

3. Weigh the mass accurately 

4. Then take a cleaned and dry1 L volumetric flask and place a funnel top of it. Then carefully add the salt into the volumetric flask and finally wash the funnel and watch glass with de-ionized water. That water also should be added into the volumetric flask.

5. Then add some de-ionized water into the volumetric flask and swirl well until all salt are dissolved.

<span>6. Then top up to mark of the volumetric flask carefully. 
</span>
</span>
7. As the final step prepared solution should be labelled.
4 0
2 years ago
How much energy is required to raise the temperature of 10.6 grams of gaseous neon from
Alona [7]

Answer:

Approximately 1.95 \times 10^{2}\; \rm J.

Explanation:

Look up the specific heat of gaseous neon:

c = 1.03 \; \rm J \cdot g^{-1} \cdot K^{-1}.

Calculate the required temperature change:

\Delta T = (37.9 - 20.0)\; \rm K = 17.9\; \rm K.

Let m denote the mass of a sample of specific heat C. Energy required to raise the temperature of this sample by \Delta T:

Q = c \cdot m \cdot \Delta T.

For the neon gas in this question:

  • c = 1.03\; \rm J \cdot g^{-1}\cdot K^{-1}.
  • m = 10.6\; \rm g.
  • \Delta T = (37.9 - 20.0)\; \rm K = 17.9\; \rm K.

Calculate the energy associated with this temperature change:

\begin{aligned}Q &= c \cdot m \cdot \Delta T \\ &= 1.03\; \rm J \cdot g^{-1}\cdot K^{-1} \times 10.6\; \rm g \times 17.9\; \rm K \\ &\approx 1.95 \times 10^{2}\; \rm J\end{aligned}.

3 0
3 years ago
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