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UkoKoshka [18]
3 years ago
5

For #11 how to determine the signs?

Chemistry
2 answers:
vladimir1956 [14]3 years ago
6 0
They a all positive bro
Viefleur [7K]3 years ago
3 0
The first reaction is exothermic as it releases heat as shown by the '+ 48 kJ'. When a reaction is exothermic the enthalpy change (ΔH) is negative as the system is losing heat. The entropy change (ΔS) is also negative as 4 moles of gas are reacting to form 2 moles of gas, reducing the disorder in the system. Since the spontaneity of a reaction is governed by ΔG = ΔH - TΔS, where ΔG must be negative for a spontaneous reaction, the reaction is only spontaneous at low temperatures as both ΔH and ΔS are negative, so as temperature increases, so does ΔG, toward 0.
The second reaction is endothermic as it absorbs heat therefore having a positive ΔH, and a positive ΔS as one mole of liquid is converted to one mole of more disordered gas. Using the same equation as before it can be shown that the reaction is only spontaneous at higher temperatures. These answers all hold true for the 3rd reaction as well (i.e. positive ΔH, positive ΔS and spontaneous at high temperatures).
Finally, reaction 4 is exothermic, therefore negative ΔH, and has a positive ΔS as 2 moles in solution are produced from one mole of solid. Therefore using the equation shown before, ΔG will always be negative regardless of temperature, and therefore the reaction is always spontaneous.
Hope this helps! If you could I would greatly appreciate you making this the brainliest answer :) If you have any questions feel free to ask.

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sladkih [1.3K]

Answer:

When we cook food in the kitchen, that's the region of higher concentration of the smell. By diffusion, the smell spreads to the whole room and thereby whole house, so anyone standing at a distance, can smell it.

5 0
2 years ago
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Please help me..!!!!!!!!!!!!!
Viefleur [7K]

Answer:

The answer you selected is correct (A)have

Explanation:

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5 0
2 years ago
Which energy profile best shows that the enthalpy of formation of CS2 is 89.4 KJ/mol?
Anna11 [10]

Answer:

Option C. Energy Profile D

Explanation:

Data obtained from the question include:

Enthalpy change ΔH = 89.4 KJ/mol.

Enthalpy change (ΔH) is simply defined as the difference between the heat of product (Hp) and the heat of reactant (Hr). Mathematically, it is expressed as:

Enthalpy change (ΔH) = Heat of product (Hp) – Heat of reactant (Hr)

ΔH = Hp – Hr

Note: If the enthalpy change (ΔH) is positive, it means that the product has a higher heat content than the reactant.

If the enthalpy change (ΔH) is negative, it means that the reactant has a higher heat content than the product.

Now, considering the question given, the enthalpy change (ΔH) is 89.4 KJ/mol and it is a positive number indicating that the heat content of the product is higher than the heat content of the reactant.

Therefore, Energy Profile D satisfy the enthalpy change (ΔH) for the formation of CS2 as it indicates that the heat content of product is higher than the heat content of the reactant.

7 0
3 years ago
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Someone please answer
BARSIC [14]

1) 100s of millions of years ago Trees and plants fall into swamps

2) Layers of rotting plant matter builds up underwater

3) Over millions of years the weight of layers heat the plant matter and turn into Peat

4) Over millions of years more pressure and heat turns Peat into coal

5 0
2 years ago
1,5,25,125 what’s the pattern rule and extend by 3 more numbers
nika2105 [10]

For the first one the pattern is multiply the previous number by five as you see 1 x 5 = 5 and so on. To keep adding to it you would do

125 x 5 = 625     625 x 5 = 3125    3125 x 5 = 15625

Now for the second one the pattern is divide the previous number by three as you can see 2187 / 3 = 729 and so on. To keep going you would

81 / 3 = 27       27 / 3 = 9        9 / 3 = 3

I hope this helps you and if you have anymore questions i'll be  glad to answer them.



4 0
3 years ago
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