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alexandr1967 [171]
3 years ago
5

A sample of hydrogen occupies a volume of 351 mL at a temperature of 20 degrees Celsius. What is the new volume if the temperatu

re increases to 38 degrees Celsius? (Do not forget to convert to Kelvin!)
Chemistry
1 answer:
xeze [42]3 years ago
6 0
Volume of Hydrogen V1 = 351mL 
Temperature T1 = 20 = 20 + 273 = 293 K 
Temperature T2 = 38 = 38 + 273 = 311 K 
We have V1 x T2 = V2 x T1 
So V2 = (V1 x T2) / T1 = (351 x 311) / 293 = 372.56 
Volume at 38 C = 373 ml
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Answer:

1.Backward

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4.Forward

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When we increase the temperature

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Using Lechatelier principle

1.The equilibrium shift in backward direction when we increase the temperature.

2.When we add CaO then it is not reactant of given reaction or not a product therefore, when we add CaO then it does not effect euilibrium condition.

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Hence , the reaction would be favored backward  if the amount of chlorine gas was decreased.

4.When we increase the pressure then the equilibrium shift in forward direction.

Hence, the reaction would be favored in forward reaction when we increase the pressure.

5.When we increase concentration of any  reactant then the equilibrium shift in forward direction.

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3 years ago
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Answer:

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Answer:

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Substituting the given values, we get –  

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Delta G is negative hence the process is spontaneous and will not violate the second law of thermodynamics

(b) DeltaH = -84 kj mol-2 (-20 kcal mol-1), DeltaS = -125j mol-2K-1)(-30 cal mol-1 K-1)

Delta G =-84 -298 *(-125/1000) = -46.75 KJ/mol

Delta G is negative hence the process is spontaneous and will not violate the second law of thermodynamics

(c) DeltaH = +84 kj mol-2 (+20 kcal mol-1), DeltaS = +125j mol-2K-1)(+30 cal mol-1 K-1)

Delta G = 84 -298 *(125/1000) = +46.75 KJ/mol

Delta G is positive hence the process is non-spontaneous and will violate the second law of thermodynamics

(d) DeltaH = +84 kj mol-2 (+20 kcal mol-1), DeltaS = +125j mol-2K-1)(-30 cal mol-1 K-1)

Delta G = 84 -298 *(-125/1000) = + 121.25  KJ/mol

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