1 mole of H2O is produced Oxygen is completely consumed Open in App 6 Text Solution 1.0 mole of `H_(2)O` is produced1.0 mole of NO will be producedall the oxygen will be consumedall the ammonia will be consumed Answer : C Solution : `underset(" 4 mol")(4NH_(3)(g))+underset("5 mol")(5O_(2)(g))tounderset("4 mol")(4NO(g))+underset("6 mol")(6H_(2)O(1))` <br> According to equation , <br> 5 moles of `O_(2)` required = 4 moles of ` NH_(3)` <br> 1 mole of `O_(2)` requires `=(4)/(5)=0.8` mole of `NH_(3)` While 1 mole of `NH_(3)` requires `=(5)/(4) = 1.25 " moles of " O_(2)` <br> As there is 1 mole of `NH_(3)` and 1 mole of `O_(2)` , so all the oxygen will be consumed . |