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3 years ago

What does the second law of thermodynamics say about entropy?

Chemistry

2 answers:

Annette [7]3 years ago

8 0

Answer:

the ansnwer is c mf kf n dsj njnr kgjrk nj ee h ewfkjhnf ewjn fnkwfnjnfnfunf

Explanation:

because is sooo goood

rodikova [14]3 years ago

4 0

Answer:

The second law of thermodynamics states that the total entropy of an isolated system can never decrease over time, and is constant if and only if all processes are reversible.

Explanation:

Isolated systems spontaneously evolve towards thermodynamic equilibrium, the state with maximum entropy. hope this helps you :)

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Please help! will give brainliest!!

Varvara68 [4.7K]

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4 0

3 years ago

F2(g)+2Br(aq)=Br(t)+F(aq) which species is redused? a)F b)Br c)F2 d)Br2

ololo11 [35]

The Answer For Your Question is:

A) F

4 0

3 years ago

What is the volume of an 2.3 solution with 212 grams of calcium chloride dissolved in it

Travka [436]

830 mL. A 2.3 mol/L solution of CaCl2 has a volume of 830 mL

I am guessing that the concentration of your solution is 2.3 mol/L.

a) Moles of CaCl2

MM of CaCl2 = 110.98 g/mol

Moles of CaCl2 = 212 g CaCl2 x (1 mol CaCl2/110.98 g CaCl2)

= 1.910 mol CaCl2

b) Volume of solution

V = 1.910 mol CaCl2 x (1 L solution/2.3 mol CaCl2) = 0.83 L solution

= 830 mL solution

5 0

3 years ago

While ethanol is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting e

sp2606 [1]

The question is incomplete, here is the complete question:

While ethanol is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene with water vapor at elevated temperatures.

A chemical engineer studying this reaction fills a 1.5 L flask at 12°C with 1.8 atm of ethylene gas and 4.7 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.16 atm of ethylene gas and 4.06 atm of water vapor.

The engineer then adds another 1.2 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.

Answer: The partial pressure of ethanol after equilibrium is reached the second time is 1.0 atm

Explanation:

We are given:

Initial partial pressure of ethylene gas = 1.8 atm

Initial partial pressure of water vapor = 4.7 atm

Equilibrium partial pressure of ethylene gas = 1.16 atm

Equilibrium partial pressure of water vapor = 4.06 atm

The chemical equation for the reaction of ethylene gas and water vapor follows:

$CH_2CH_2(g)+H_2O(g)\rightleftharpoons CH_3CH_2OH(g)$

Initial: 1.8 4.7

At eqllm: 1.8-x 4.7-x

Evaluating the value of 'x'

$\Rightarrow (1.8-x)=1.16\\\\x=0.64$

The expression of $K_p$ for above equation follows:

$K_p=\frac{p_{CH_3CH_2OH}}{p_{CH_2CH_2}\times p_{H_2O}}$

$p_{CH_2CH_2}=1.16atm\\p_{H_2O}=4.06atm\\p_{CH_3CH_2OH}=0.64atm$

Putting values in above expression, we get:

$K_p=\frac{0.64}{1.16\times 4.06}\\\\K_p=0.136$

When more ethylene is added, the equilibrium gets re-established.

Partial pressure of ethylene added = 1.2 atm

$CH_2CH_2(g)+H_2O(g)\rightleftharpoons CH_3CH_2OH(g)$

Initial: 2.36 4.06 0.64

At eqllm: 2.36-x 4.06-x 0.64+x

Putting value in the equilibrium constant expression, we get:

$0.136=\frac{(0.64+x)}{(2.36-x)\times (4.06-x)}\\\\x=0.363,13.41$

Neglecting the value of x = 13.41 because equilibrium partial pressure of ethylene and water vapor will become negative, which is not possible.

So, equilibrium partial pressure of ethanol = (0.64 + x) = (0.64 + 0.363) = 1.003 atm

Hence, the partial pressure of ethanol after equilibrium is reached the second time is 1.0 atm

3 0

3 years ago

Indicate how you might prepare acetic acid from ethene

ruslelena [56]

Acetic acid can be prepared from ethane by oxidizing it. Acetic acid is generally a carboxylic acid. These acids can be made by the oxidation of alcohols using potassium dichromate(VI) solution with sulfuric acid. Ethane is made into acetic acid in two steps. First it is formed into an aldehyde and then to acetic acid.

8 0

3 years ago