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Ammonium nitrite decomposes to give off nitrogen gas and liquid water. How many grams of ammonium nitrite must have reacted if 2.58 L of gas was collected over water in a gas collecting tube at 21.0°C and 97.8 kPa?

Balanced equation:


Ans to 3:


(6 pts) Will the volume of nitrogen (from the previous problem) INCREASE, DECREASE or remain the SAME if... *Explain briefly*


...the experiment is done at significantly higher temperature?

B. ...the amount of ammonium nitrite was increased?


C.

...the experiment was not collected over water?

Ammonium nitrite decomposes to give off nitrogen gas and liquid water How many grams of ammonium nitrite must have reacted if 2 58 L of

Answer :

The ammonium nitrite that we are going to use is 6.4 g.

To use stoichiometry

The law of conservation of mass, is the basis of what we ant to do in the solving of the task that is at hand., is the foundation of stoichiometry. As a result, the total mass of the reactants and the total mass of the products must match.

The reaction's equation is;

[NH4]NO2 N2 + 2H2O

There is pressure would be 95.3 kPa, or 0.94 atm

PV = nRT

n = PV/RT

n = 0.94 * 2.58/0.082 * 294

n=0.1 moles.

Mass of the ammonium nitrite is; if the reaction is 1:1.

64 g/mol * 0.1 moles

Learn more about stoichiometry:https://brainly.com/question/30218216

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