#320# #g# of solid ammonium nitrite, #NH_4NO_2#, decomposes when heated according to the balanced equation: #NH_4NO_2 - N_2+2H_2O#. What total volume of gases at #819# #K# is emitted by this reaction?

Question

#320# #g# of solid ammonium nitrite, #NH_4NO_2#, decomposes when heated according to the balanced equation: #NH_4NO_2 -> N_2+2H_2O#. What total volume of gases at #819# #K# is emitted by this reaction?

Serenity Allen · Accepted Answer

Each mole of #NH_4NO_2# produces #3# #mol# of gases total (#N_2# and #H_2O#), and we have #5# #mol#. So #3xx5 = 15# #mol# of gas at STP is #336# #L#. Converting to #819# #K# gives a volume of #1008# #L#.

The molar mass of #NH_4NO_2# is #64# #gmol^-1# (two #N# at #14#, four #H# at #1#, two #O# at #16#). Find the number of moles of #NH_4NO_2#: #n=m/M=320/64=5# #mol# From the balanced equation, each mole of #NH_4NO_2# yields 1 mole of #N_2# and 2 moles of #H_2O# (which is definitely a gas at #819# #K#), for a total of 3 moles of gas. For ideal gases (which we can treat these real gases as for our purposes), 1 mole of any gas at STP (#273# #K# and #1# #atm#) occupies #22.4# #L#. That means we have #3xx5 = 15# #mol# of product gases, and they occupy a volume of #336# #L# at STP. We need to change the temperature from #273# #K# to #819# #K#, and the pressure stays the same at #1# #atm#, so: #V_1/T_1=V_2/T_2# Organizing: #V_2=V_1T_2/T_1 = 336 xx 819/273 = 1008# #L#

Serenity Allen · Answer

undefined The molar mass of ammonia nitrite (NH4NO2) is 80.05 g/mol. To find the moles of gases produced, we first need to find the number of moles of NH4NO2 decomposed; moles = mass / molar mass moles = 320 g / 80.05 g/mol = 3.997 moles. Based on the balanced equation, 1 mole of NH4NO2 produces 1 mole of N2 and 2 moles of H2O, so moles of gases produced = 1 mole (N2) + 2 moles (H2O) = 3 moles. Next, we need to use the ideal gas law to calculate the volume of gases at 819 K. Here, PV = nRT. Where: P = pressure (assumed to be 1 atm) V = volume (unknown) n = number of moles (3 moles) R = ideal gas constant (0.0820

#320# #g# of solid ammonium nitrite, #NH_4NO_2#, decomposes when heated according to the balanced equation: #NH_4NO_2 -&gt; N_2+2H_2O#. What total volume of gases at #819# #K# is emitted by this reaction?

#320# #g# of solid ammonium nitrite, #NH_4NO_2#, decomposes when heated according to the balanced equation: #NH_4NO_2 -> N_2+2H_2O#. What total volume of gases at #819# #K# is emitted by this reaction?