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kow [346]
3 years ago
13

If you add salt continuously to a glass of water, eventually some salt will remain at the bottom. why?

Chemistry
2 answers:
nadya68 [22]3 years ago
5 0
If you keep adding salt, the amount of salt and water will eventually pass equilibrium (for which every water molecule has a salt). This results in the remaining salt not being able to dissociate. 
GREYUIT [131]3 years ago
3 0
Http://www.lcmrschooldistrict.com/demers/cbphysicalscience/Chp%208-3%20Solubility%20and%20Concentrat...

This website helped me understand the concept.
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14) A wavelength of radiation has a frequency of 2.10 x 1014 Hz. What is the wavelength of this radiation in nm, and
Evgesh-ka [11]

Answer:

λ = 1.43 x 10³ meters (radio waves)

Explanation:

c = f·λ => λ = c/f

λ = wavelength = ?

f = frequency = 2.10 x 10¹⁴ Hz = 2.10 x 10¹⁴ cycles/sec

c = speed of light (vacuum) = 3.0 x 10⁸m/sec

λ = c/f = 3.0 x 10⁸m/sec / 2.10 x 10¹⁴sec⁻¹ = 1.43 x 10³ meters (radio waves)

3 0
3 years ago
Which of the following is not a clue that a chemical reaction has taken place? *
DaniilM [7]

Answer:

A pure solid is heated and turns into a pure liquid.

Explanation:

No colour change recorded, only change of state, hence this is a physical change - physical changes I.e. change of state and temperature are not chemical reactions.

7 0
3 years ago
2C2H2(g)+5O2(g)=4CO2(g)+2H2O(g)
balandron [24]

The volume of ethyne, C₂H₂ required to produce 12 moles of CO₂ assuming the reaction is at STP is 134.4 L

<h3>Balanced equation</h3>

2C₂H₂(g) + 5O₂(g) --> 4CO₂(g) + 2H₂O(g)

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

<h3>How to determine the mole of C₂H₂ needed to produce 12 moles of CO₂</h3>

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

Therefore,

12 moles of CO₂ will be produce by = (12 × 2) / 4 = 6 moles of C₂H₂

<h3>How to determine the volume (in L) of C₂H₂ needed at STP</h3>

At standard temperature and pressure (STP),

1 mole of C₂H₂ = 22.4 L

Therefore,

6 moles of C₂H₂ = 6 × 22.4

6 moles of C₂H₂ = 134.4 L

Thus, we can conclude that the volume of C₂H₂ needed for the reaction at STP is 134.4 L

Learn more about stoichiometry:

brainly.com/question/14735801

#SPJ1

3 0
2 years ago
What are the terms that descripe these values for the element oxygen?
Serga [27]

Answer:

16 is the mass number. 8 is the atomic number.

5 0
2 years ago
What is the pressure in a 5.00 L tank with<br> 7.10 moles of oxygen at 39.3 °C?
Katena32 [7]

Answer:

36.4 atm

Explanation:

To find the pressure, you need to use the Ideal Gas Law. The equation looks like this:

PV = nRT

In this equation,

-----> P = pressure (atm)

-----> V = volume (L)

-----> n = moles

-----> R = constant (0.0821 L*atm/mol*K)

-----> T = temperature (K)

Before you can plug the given values into the equation, you first need to convert Celsius to Kelvin.

P = ? atm                         R = 0.0821 L*atm/mol*K

V = 5.00 L                       T = 393 °C + 273.15 = 312.45 K

n = 7.10 moles

PV = nRT

P(5.00 L) = (7.10 moles)(0.0821 L*atm/mol*K)(312.45 K)

P(5.00 L) = 182.130

P = 36.4 atm

8 0
1 year ago
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