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2 years ago

Use the drop-down menus to complete the sentences describing what happens when the temperature of a fluid

Chemistry

2 answers:

Anton [14]2 years ago

8 0

Answer:

increases

decreases

rises

Explanation:

Scorpion4ik [409]2 years ago

5 0

when the temperature of a fluid increases the kinetic energy of the molecules increases.

<u>Explanation:</u>

when there is a change in liquid temperature then there will be changes in its properties especially in the (KE) kinetic energy of molecules and the density of the fluid.
Due to the addition of the heat kinetic energy of the fluid molecules as it gains the heat, the intermolecular movement increases so there will be in the increased collision between the molecules which results in breaking the intermolecular force.
Whenever the heat is applied to any matters nature is to tend to expand so the fluids also expand which results in the decrease in the density of the liquid.
And also due to the increases in the kinetic energy, the speed of the fluid also increases.

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Vaporization is an endothermic process. Using the terms 'kinetic energy' and 'intermolecular forces', explain how the addition o

Novay_Z [31]

An endothermic process is a process that needs energy in order to proceed. This is the opposite of exothermic which is a process of releasing energy. During an endothermic process, the temperature of the system is increased thus exciting the molecules and allowing them to move faster. This will cause liquid to vaporize.

5 0

3 years ago

Propane burns in oxygen to produce carbon dioxide and water what is the percent yeild

amid [387]

Answer:

The percentage yield is 78.2g

Explanation:

Given, mass of propane = 42.8 g , sufficient O2 percent yield = 61.0 % yield.

Reaction - C3H8(g)+5O2(g)------> 3CO2(g)+4H2O(g)

First we need to calculate the moles of propane

Moles of propane = $\frac{42.8}{44.096}$ g.mol-1

= 0.971 moles

So, moles of CO2 from the moles of propane

1 mole of C3H8(g) = 3 moles of CO2(g)

So, 0.971 moles of C3H8(g) = ?

= 2.913 moles of CO2

So theoretical yield = 2.913 moles $\times$ 44.0 g/mol

= 128.2 g

So, the actual mass of CO2 = percent yield $\times$ theoretical yield / 100 %

= 61.0 % $\times$ 128.2 g / 100 %

= 78.2 g

the mass of CO2 that can be produced if the reaction of 42.8 g of propane and sufficient oxygen has a 61.0 % yield is 78.2 g

4 0

2 years ago

What is the pH of a solution when the [OH - ] = 1 x 10 -3

dsp73

Answer:

The pH is 11

Explanation:

Because pH + pOH = 14

and pOH = - log [OH⁻] = - log (1 x 10⁻³) = 3

we can now calculate pH by manipulating equation one above

pH = 14 - pOH = 14 - 3 = 11

Thus the pH of the solution is 11

8 0

3 years ago

A 1 liter solution contains 0.247 M nitrous acid and 0.329 M sodium nitrite. Addition of 0.271 moles of calcium hydroxide will:

Inessa05 [86]

Answer:

a. Raise the pH slightly

Explanation:

We know that

Pka of HNO2/KNO2 =3.39

Moles of HNO2 in the buffer=0.247 mol/L×1L=0.247 moles

Moles of NO2-=0.329mol/L×1L=0.329 moles

If 0.271 moles of Ca(OH)2 is added it will neutralise 0.136 moles of acid ,HNO2,remaining HNO2=0.247-0.136=0.111 moles

Moles of NO2- will increase as 0.0333 moles Ca(NO)2 will be formed =0.0333+0.036=0.0693 moles

pH=pka+log [base]/[acid] {henderson -hasselbach equation}

=3.39+log (0.0693/0.0317)=3.39+0.34=3.73

pH=3.73

4 0

3 years ago

15.50 g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.50 g AgCl is produced. what is the theoretical yield of AgCl

Readme [11.4K]

Answer:

The answer to your question is 41.6 g of AgCl

Explanation:

Data

mass of NH₄Cl = 15.5 g

mass of AgNO₃ = excess

mass of AgCl = 35.5 g

theoretical yield = ?

Process

1.- Write the balanced chemical reaction.

NH₄Cl + AgNO₃ ⇒ AgCl + NH₄NO₃

2.- Calculate the molar mass of NH₄Cl and AgCl

NH₄Cl = 14 + 4 + 35.5 = 53.5 g

AgCl = 108 + 35.5 = 143.5 g

3.- Calculate the theoretical yield

53.5 g of NH₄Cl -------------------- 143.5 g of AgCl

15.5 g of NH₄Cl ------------------- x

x = (15.5 x 143.5) / 53.5

x = 2224.25 / 53.5

x = 41.6 g of AgCl

8 0

2 years ago