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kari74 [83]
3 years ago
8

Which factor has the least effect on the rate of solution of a solid in a liquid?

Chemistry
2 answers:
vitfil [10]3 years ago
4 0
The pressure will not affect the rate of solution.
ziro4ka [17]3 years ago
3 0

Answer: Option (c) is the correct answer.

Explanation:

Since, the substance added is a solid and particles of a solid are very closely held to each other because of strong intermolecular forces of attraction between them.

This makes them to have a definite shape and volume. Therefore, when pressure is applied on a solid then its particles will be least affected by it as they are already close to each other.

Whereas stirring, amount of surface area, and temperature will equally affect the rate of dissolution of the solid.

Hence, we can conclude that pressure is the factor that has least effect on the rate of solution of a solid in a liquid.

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If you are given an ideal gas with pressure (P) = 259,392.00 Pa and temperature (T) = 2.00 oC of 1 mole Argon gas in a volume of
3241004551 [841]

Answer:

 R = 0.064 dm³ atm K⁻¹ mol⁻¹

Explanation:

Answer:

Explanation:

Data Given:

volume of gas V = 8.8 dm³

no. of mole of gas (n) = 1 mole

Pressure P = 259,392.00 Pa  

Convert Pascal (Pa) to atm (atmospheric pressure)

As

101,325 Pascals = 1 atm

So,

259,392.00 Pa  = 2 atm

Then Pressure (P) = 2 atm

Temperature T = 2.00 °C  

change the temperature from °C to K

As  to convert °C to K the below formula used

                   0°C + 273.15 = 273.15K

So, for 2 °C

                    2°C  + 273.15 =  275.15 K

So,

Temperature T  = 275.15 K

ideal gas constant = ?

formula used for Ideal gases

                            PV = nRT

as we have to find R of the gas:

we will rearrange the ideal gas equation as below:

R = PV / nT ........................................... (1)

Put value in equation (1)

                 R = 2atm x 8.8 dm³ / 1 mole x 275.15 K

                  R = 17.6 atm. dm³ / 275.15 mol. K

                  R = 0.064 dm³ atm K⁻¹ mol⁻¹

So the value of R is 0.064 dm³ atm K⁻¹ mol⁻¹

and the unit of R (ideal gas constant) is dm³ atm K⁻¹ mol⁻¹

7 0
3 years ago
Ca(OH)2 + H2SO4 ⟶2H2O + CaSO4 What volume of 1.45 M Ca(OH)2 is needed to react with 25.0 moles of H2SO4?
Shkiper50 [21]

Answer:

We need 17.2 L of Ca(OH)2

Explanation:

Step 1: Data given

Concentration of Ca(OH)2 = 1.45 M

Moles of H2SO4 = 25.0 moles

Step 2: The balanced equation

Ca(OH)2 + H2SO4 ⟶2H2O + CaSO4

Step 3: Calculate moles Ca(OH)2

For 1 mol Ca(OH)2 we need 1 mol H2SO4 to produce 2 moles H2O and 1 mol CaSO4

For 25.0 moles H2SO4 we'll need 25.0 moles Ca(OH)2 to produce 50 moles H2O and 25.0 moles CaSO4

Step 4: Calculate volume of Ca(OH)2

Volume Ca(OH)2 = moles Ca(OH)2 / concentration Ca(OH)2

Volume Ca(OH)2 = 25.0 moles / 1.45 M

Volume Ca(OH)2 = 17.2 L

We need 17.2 L of Ca(OH)2

3 0
3 years ago
What observation about light supported Einstein's theory?
Llana [10]

In 1905 Albert Einstein had proposed a solution to the problem of observations made on the behaviour of light having characteristics of both wave and particle theory. From work of Plank on emission of light from hot bodies, Einstein suggested that light is composed of tiny particles called <span>photons, </span>and each photon has energy.

Light theory branches in to the physics of <span>quantum mechanics, </span>which was conceptualised in the twentieth century. Quantum mechanics deals with behaviour of nature on the atomic scale or smaller.

As a result of quantum mechanics, this gave the proof of the dual nature of light and therefore not a contradiction.

5 0
3 years ago
Which of the following is a reduction half-reaction?
Marta_Voda [28]

Solution : An oxidation reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between tow species an oxidaion reductin reaction is any chemical reaction in which the oxidation number of a molecule atom or ion changes by gaining or losing an electron

3 0
3 years ago
This is agree or disagree I need help ASAP!!
PIT_PIT [208]
All of them are agree :)
8 0
2 years ago
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