At 2730 °C, hydrogen molecules dissociate into hydrogen atoms according to the equation H2 (g) →...

At 2730 °C, hydrogen molecules dissociate into hydrogen atoms according to the equation H2 (g) → 2 H(g). 10.0 g H2 (g) is placed into a 100.0-L container, sealed and heated to 2730 °C so that the hydrogen molecules begin to dissociate. What is the partial pressure of hydrogen molecules and the total pressure within the container once 25% of H2 has dissociated?

The answers are PH2 = 9.2 atm, Ptotal = 15 atm, but how I get it?

Expert Solution

queen_honey_blossom answered 2 years ago

At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g)2HI(g)↽−−⇀H2(g)+I2(g) For HI(g)HI(g) heated to 500 °C in...

At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g)2HI(g)↽−−⇀H2(g)+I2(g) For HI(g)HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2]=0.400 M[H2]=0.400 M , [I2]=0.400 M[I2]=0.400 M , and [HI]=3.38 M[HI]=3.38 M . If an additional 1.00 mol of HI(g)HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI]= [H2]= [I2]= Please help and show work!

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