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3.2 moles of HI were heated in a sealed bulb at 444 degree celcius till the equilibrium was reached. Its degree of dissociation was found to be 20%.Calculate the no. of moles of hydrogen iodide, hydrogen, and iodine present at the equilibrium point and determine the value of equilibrium constant for the reaction 2HI(g) gives H2(g) I2(g). Considering the volume of the container 1 Litre.? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 3.2 moles of HI were heated in a sealed bulb at 444 degree celcius till the equilibrium was reached. Its degree of dissociation was found to be 20%.Calculate the no. of moles of hydrogen iodide, hydrogen, and iodine present at the equilibrium point and determine the value of equilibrium constant for the reaction 2HI(g) gives H2(g) I2(g). Considering the volume of the container 1 Litre.? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 3.2 moles of HI were heated in a sealed bulb at 444 degree celcius till the equilibrium was reached. Its degree of dissociation was found to be 20%.Calculate the no. of moles of hydrogen iodide, hydrogen, and iodine present at the equilibrium point and determine the value of equilibrium constant for the reaction 2HI(g) gives H2(g) I2(g). Considering the volume of the container 1 Litre.?.

Solutions for 3.2 moles of HI were heated in a sealed bulb at 444 degree celcius till the equilibrium was reached. Its degree of dissociation was found to be 20%.Calculate the no. of moles of hydrogen iodide, hydrogen, and iodine present at the equilibrium point and determine the value of equilibrium constant for the reaction 2HI(g) gives H2(g) I2(g). Considering the volume of the container 1 Litre.? in English & in Hindi are available as part of our courses for NEET. Download more important topics, notes, lectures and mock test series for NEET Exam by signing up for free.

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