Answer:
The reaction will be spontaneous
Explanation:
To determine if the reaction will be spontaneous or not at this temperature, we need to calculate the Gibbs's energy using the following formula:
<u>If the Gibbs's energy is negative, the reaction will be spontaneous, but if it's positive it will not.</u>
Calculating the 
:
Now, other factor we need to determine is the sign of the S variation. When talking about gases, the more moles you have in your system the more enthropic it is.
In this reaction you go from 7 moles to 8 moles of gas, so you can say that you are going from one enthropy to another higher than the first one. This results in: ![\Delta S>0[/tex}Back to this expression: [tex]\Delta G= -1267 - 473 K* \Delta S](https://tex.z-dn.net/?f=%5CDelta%20S%3E0%5B%2Ftex%7D%3C%2Fp%3E%3Cp%3EBack%20to%20this%20expression%3A%20%3C%2Fp%3E%3Cp%3E%5Btex%5D%5CDelta%20G%3D%20-1267%20-%20473%20K%2A%20%5CDelta%20S%20)
If the variation of S is positive, the Gibbs's energy will be negative always and the reaction will be spontaneous.
Answer:
use google and use the first link
Explanation:
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Correct Answer:
Option 3 i.e. 30 g of KI dissolved in 100 g of water.
Reason:
Depression in freezing point is a
colligative property and it is directly proportional to molality of solution.
Molality of solution is mathematically expressed as,
Molality = </span>
<span>
In case of
option 1 and 2, molality of solution is
0.602 m. For
option 3, molality of solution is
1.807 m, while in case of
option 4, molality of solution is
1.205 m.
<u><em>Thus, second solution (option 2) has highest concentration (in terms of molality). Hence, it will have lowest freezing point</em></u></span>
Answer:
1.62 L
Explanation:
T= 97+273.15= 370.15
R= 0.08206 atm/mol⋅K
V= 45 L
n= 2.4 mol
P= (n⋅R⋅T)/V
= (2.4 x 0.08206 x 370.15)/(45) = 1.61997 = 1.62
