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Question: Given below are some molecules CH3COONH4(s), (NH4)2Cr2O7, (NH4)2SO4, Ba(N3)2, NaNO2, NaN3, NH4NO2, N...

Given below are some molecules CH3COONH4(s), (NH4)2Cr2O7, (NH4)2SO4, Ba(N3)2, NaNO2, NaN3, NH4NO2, NH4NO3, NH4Cl, (NH4)2CO3

x = no. of molecules that release N₂ gas on thermal decomposition y = no. of molecules that release NH3 gas on thermal decomposition

The value of y - x is

Answer

0

Explanation

Solution

To determine the values of x and y, we need to analyze the thermal decomposition products of each given molecule.

Molecules that release N₂ gas on thermal decomposition (x):

  1. (NH₄)₂Cr₂O₇ (Ammonium dichromate): (NH4)2Cr2O7(s)→ΔCr2O3(s)+N2(g)+4H2O(g)\text{(NH}_4\text{)}_2\text{Cr}_2\text{O}_7(\text{s}) \xrightarrow{\Delta} \text{Cr}_2\text{O}_3(\text{s}) + \text{N}_2(\text{g}) + 4\text{H}_2\text{O}(\text{g}) Releases N₂.

  2. Ba(N₃)₂ (Barium azide): Ba(N3)2(s)→ΔBa(s)+3N2(g)\text{Ba(N}_3\text{)}_2(\text{s}) \xrightarrow{\Delta} \text{Ba}(\text{s}) + 3\text{N}_2(\text{g}) Releases N₂.

  3. NaN₃ (Sodium azide): 2NaN3(s)→Δ2Na(s)+3N2(g)2\text{NaN}_3(\text{s}) \xrightarrow{\Delta} 2\text{Na}(\text{s}) + 3\text{N}_2(\text{g}) Releases N₂.

  4. NH₄NO₂ (Ammonium nitrite): NH4NO2(s)→ΔN2(g)+2H2O(g)\text{NH}_4\text{NO}_2(\text{s}) \xrightarrow{\Delta} \text{N}_2(\text{g}) + 2\text{H}_2\text{O}(\text{g}) Releases N₂.

Molecules that do NOT release N₂ gas (primarily) or NH₃ gas:

  • NaNO₂ (Sodium nitrite): Thermally stable. Decomposes at very high temperatures, not releasing N₂ or NH₃.
  • NH₄NO₃ (Ammonium nitrate): Primarily decomposes to nitrous oxide (N₂O) at moderate temperatures. NH4NO3(s)→ΔN2O(g)+2H2O(g)\text{NH}_4\text{NO}_3(\text{s}) \xrightarrow{\Delta} \text{N}_2\text{O}(\text{g}) + 2\text{H}_2\text{O}(\text{g}) Does not release N₂ as the characteristic decomposition product.

Therefore, the number of molecules that release N₂ gas, x = 4.

Molecules that release NH₃ gas on thermal decomposition (y):

  1. CH₃COONH₄(s) (Ammonium acetate): CH3COONH4(s)→ΔCH3COOH(g)+NH3(g)\text{CH}_3\text{COONH}_4(\text{s}) \xrightarrow{\Delta} \text{CH}_3\text{COOH}(\text{g}) + \text{NH}_3(\text{g}) Releases NH₃.

  2. (NH₄)₂SO₄ (Ammonium sulfate): (NH4)2SO4(s)→Δ2NH3(g)+H2SO4(g)\text{(NH}_4\text{)}_2\text{SO}_4(\text{s}) \xrightarrow{\Delta} 2\text{NH}_3(\text{g}) + \text{H}_2\text{SO}_4(\text{g}) Releases NH₃.

  3. NH₄Cl (Ammonium chloride): NH4Cl(s)→ΔNH3(g)+HCl(g)\text{NH}_4\text{Cl}(\text{s}) \xrightarrow{\Delta} \text{NH}_3(\text{g}) + \text{HCl}(\text{g}) Releases NH₃.

  4. (NH₄)₂CO₃ (Ammonium carbonate): (NH4)2CO3(s)→Δ2NH3(g)+CO2(g)+H2O(g)\text{(NH}_4\text{)}_2\text{CO}_3(\text{s}) \xrightarrow{\Delta} 2\text{NH}_3(\text{g}) + \text{CO}_2(\text{g}) + \text{H}_2\text{O}(\text{g}) Releases NH₃.

Therefore, the number of molecules that release NH₃ gas, y = 4.

Calculation of y - x: y - x = 4 - 4 = 0.