`NH_(3)` is heated at `15` at, from `25^(@)C` to `347^(@)C` assuming volume constant. The new pressure becomes `50` atm at equilibrium of the reaction `2NH_(3) hArr N_(2)+3H_(2)`. Calculate `%` moles of `NH_(3)` actually decomposed.

NH_(3) is heated at 15 atm, from 25^(@)C to 347^(@)C assuming volume constant. The new pressure becomes 50 atm at equilibrium of the reaction 2NH_(3) hArr N_(2)+3H_(2) . Calculate % moles of NH_(3) actually decomposed.

NH_3 is heated initially at 15 atm from 27^@C to 127^@C at constant volume.At 127^@C equilibrium is established.The new pressure at equilibrium at 127^@C becomes 30 atm for the reaction 2NH_3(g)hArrN_2(g)+3H_2(g) Then find the % of moles of NH_3 actually decomposed.

For N_(2)+3H_(3) hArr 2NH_(3)+"Heat"

For N_(2)+3H_(3) hArr 2NH_(3)+"Heat"