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Marina CMI [18]
3 years ago
7

Test Prep

Chemistry
2 answers:
Kazeer [188]3 years ago
7 0
The butterflies will leave their cocoons and make the forest such a beautiful and wonderful magnificent scene! Hope this helps! So yeah to sum it all up: butterflies will leave the cocoons. :)
Montano1993 [528]3 years ago
4 0
The cacoons will turn into perty butterflies

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A reactant and a product of nuclear fission.<br><br> A. Neutron<br> B. Gamma
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Answer:

Neutron

Explanation:

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Fat,minerals,vitamins,water which is odd one​
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A student measures out 5 mL of calcium chloride solution into a small container and 5 mL of sodium carbonate solution in another
qwelly [4]

Answer:

15.5g

Explanation:

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3 years ago
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Calculate the entropy change for a process in which 3.00 moles of liquid water at 08c is mixed with 1.00 mole of water at 100.8c
kupik [55]
The question provides the data in an incorrect way, but what the question is asking is for the entropy change when combining 3 moles of water at 0 °C (273.15 K) with 1 mole of water at 100 °C (373.15 K). We are told the molar heat capacity is 75.3 J/Kmol. We will be using the following formula to calculate the entropy change of each portion of water:

ΔS = nCln(T₂/T₁)

n = number of moles
C = molar heat capacity
T₂ = final temperature
T₁ = initial temperature

We can first find the equilibrium temperature of the mixture which will be the value of T₂ in each case:

[(3 moles)(273.15 K) + (1 mole)(373.15 K)]/(4 moles) = 298.15 K

Now we can find the change in entropy for the 3 moles of water heating up to 298.15 K and the 1 mole of water cooling down to 298.15 K:

ΔS = (3 moles)(75.3 J/Kmol)ln(298.15/273.15)
ΔS = 19.8 J/K

ΔS = (1 mole)(75.3 J/Kmol)ln(298.15/373.15)
ΔS = -16.9 J/K

Now we combine the entropy change of each portion of water to get the total entropy change for the system:

ΔS = 19.8 J/K + (-16.9 J/K)
ΔS = 2.9 J/K

The entropy change for combining the two temperatures of water is 2.9 J/K.
3 0
3 years ago
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