How many moles of ammonium nitrate (nh4no3) are required to decompose to produce 0.90 moles of water (h2o)?

The answer to your question is 0.45 moles

Explanation:

Balanced equation

                               NH₄NO₃   ⇒   N₂O  +  2H₂O

                                2 -----------  N ----------- 2

                                4 ------------ H ----------- 4

                                3 ------------ O ----------- 3

From the balanced equation we know that 1 mol of NH₄NO₃ produces 2 moles of water, so we use proportions to find the amount of NH₄NO₃ required  to produce 0.9 moles of water.

                               1 mol of NH₄NO₃ -------------  2 moles of water

                               ?                           -------------- 0.9 moles of water

Use cross multiplication

                               x =

Simplification

                               x = 0.9 / 2

Result

                               x = 0.45 moles of NH₄NO₃

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

i think its 100.

hope this !