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Question 1(a) (i), (ii), (iii) from image INQ1 and please help me with this part too...(a) (I) from image INQ2  Why was it adequate to absorb the iodine at roorn temperature although its amount at high temperature of the experiment was actually required?

Question 1(a) (i), (ii), (iii) from image INQ1 and please help me with this part too...(a) (I) from image INQ2  Why was it adequate to absorb the iodine at roorn temperature although its amount at high temperature of the experiment was actually required?

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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Question 1(a) (i), (ii), (iii) from image INQ1 and please help me with this part too...(a) (I) from image INQ2 

Why was it adequate to absorb the iodine at roorn temperature although its amount at high temperature of the experiment was actually required?

В. PEPER TWO: STRUCTURAL QUESTIONS +12g) This equation is about the reversible reaction. 2H) Using this system as an example explain what is meant by 1) (a) equilibrium mixture ii) equilibrium constant K. ... i) It can be shown that if some radioactive iodine is added to the equilibrium mixture the iodine in the hydrogen iodide also becomes radioactive. What can be deduced from this observation? In an experiment to determine Kc, 0.210g of hydrogen iodide was heated at 800K in a bulbs of volume 100 cm until equilibrium was attained. The bulb was broken under potassium iodide solution and the iodine present found to be sufficient to react with 4.0 cm of sodium thiosulphate solution (Na2S203) of concentration0.1 moldm a) 3. -3 →21 + S,O6. 2- 2S0 + |2
Transcribed Image Text:В. PEPER TWO: STRUCTURAL QUESTIONS +12g) This equation is about the reversible reaction. 2H) Using this system as an example explain what is meant by 1) (a) equilibrium mixture ii) equilibrium constant K. ... i) It can be shown that if some radioactive iodine is added to the equilibrium mixture the iodine in the hydrogen iodide also becomes radioactive. What can be deduced from this observation? In an experiment to determine Kc, 0.210g of hydrogen iodide was heated at 800K in a bulbs of volume 100 cm until equilibrium was attained. The bulb was broken under potassium iodide solution and the iodine present found to be sufficient to react with 4.0 cm of sodium thiosulphate solution (Na2S203) of concentration0.1 moldm a) 3. -3 →21 + S,O6. 2- 2S0 + |2
In an experiment to determine Kc, 0.210g of hydrogen iodide was heated at 800k " a bulbs of volume 100 cm until equilibrium was attained. The bulb was broken under potassium iodide solution and the iodine present found to be sufficient to react with 4.0 cm of sodium thiosulphate solution (Na,S,O3) of concentration 0.1 moldm a) 3 3 -3 2S20, + 12 - 21 + S,O. Why was it adequate to absorb the iodine at room temperature although its amount at high temperature of the experiment was actually required? i) Calculate: the number of moles of hydrogen iodide in 0.210g the number of moles of iodine (12) formed in the experiment.
Transcribed Image Text:In an experiment to determine Kc, 0.210g of hydrogen iodide was heated at 800k " a bulbs of volume 100 cm until equilibrium was attained. The bulb was broken under potassium iodide solution and the iodine present found to be sufficient to react with 4.0 cm of sodium thiosulphate solution (Na,S,O3) of concentration 0.1 moldm a) 3 3 -3 2S20, + 12 - 21 + S,O. Why was it adequate to absorb the iodine at room temperature although its amount at high temperature of the experiment was actually required? i) Calculate: the number of moles of hydrogen iodide in 0.210g the number of moles of iodine (12) formed in the experiment.
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