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2 years ago

The equilibrium constant k for the synthesis of ammonia is 6.8x105 at 298 k. what will k be for the reaction at 375 k?

2 answers:

8 0

Missing in your question: ΔH= -92.22 KJ.mol^-1 and the reaction equation is :
N2(g) +3H2(g)⇄2NH3(g)
So according to this formula:
㏑(K2/K1) = -ΔH/R (1/T2 - 1/T1)
when we have ΔH= 92.22 KJ.mol^-1 & K2= X & K1= 6.8X10^5 & T1= 298 K &
T2=375 K & R constant= 8.314
So by substitution we can get the value of K2
㏑(X/6.8x10^5) = 92.22/8.314 (1/375 - 1/298)
∴X= 6.75X10^5
∴K2 = 6.75X10^5

spayn [35]2 years ago

6 0

Answer is: K be for the reaction at 375 K is 326.
Chemical reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g); ΔH = -92,22 kJ/mol.
T₁ = 298 K
T₂ = 375 K
ΔH = -92,22 kJ/mol = -92220 J/mol.
R = 8,314 J/K·mol.
K₁ = 6,8·10⁵.
K₂ = ?The van’t Hoff equation: ln(K₂/K₁) = -ΔH/R(1/T₂ - 1/T₁).
ln(K₂/6,8·10⁵) = 92220 J/mol / 8,314 J/K·mol (1/375K - 1/298K).
ln(K₂/6,8·10⁵) = 11092,13 · (0,00266 - 0,00335).
ln(K₂/6,8·10⁵) = -7,64.
K₂/680000= 0,00048
K₂ = 326,4.

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Three mixtures were prepared from three very narrow molar mass distribution polystyrene samples with molar masses of 10,000, 30,

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Answer:

(a). 46,666.7 g/mol; 78,571.4 g/mol

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Explanation:

So, we are given the molar masses for the three samples as: 10,000, 30,000 and 100,000 g mol−1.

Thus, the equal number of molecule in each sample = ( 10,000 + 30,000 + 100,000 ) / 3 = 46,666.7 g/mol.

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(b). The equal masses of each sample = 3/[ ( 1/ 10,000) + (1/30,000 ) + (1/100,000) ] = 20930.23 g/mol.

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Explanation:

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$H_{2}O(l) \rightleftharpoons H_{2}O(s)$

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A reaction in which there will be release of heat energy is known as exothermic reaction.

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Hence, phase change from liquid to solid will be exothermic in nature.

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So, when solid state of water changes into liquid state then it means energy is absorbed by the molecules of ice due to which they have gained kinetic energy. Hence, they moved away from each other leading to formation of liquid state of water.

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Specific heat of liquid water is 4.186 $J/g ^{o}C$

Specific heat of steam is 1.996 $kJ/kg/^{o}K$

Specific heat of ice is 2.1 $kJ/kg/^{o}K$

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As a result, heat will be absorbed by the liquid state of water. Hence, heat will be absorbed. Therefore, phase change from liquid to gas will be endothermic in nature.

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1 year ago

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Answer:

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