The decomposition reaction of ammonium nitrite is
1 mol ammonium nitrite produces 1 mol nitrogen and 2 mol water in gaseous state.
Given that, mass of decomposed = 128 g
Molar mass of = 2 × (At. Wt of N) + 4 × (At. Wt of H) + 2 × (At. Wt of O)
Molar mass = 2 × (14) + 4 × (1) + 2 × (16) = 64.00 g/mol
No of moles of
We already said that, 1 mol produces 1 mol and 2 mol .
Therefore 2 mol produce 2 mol and 4 mol .
Total no of moles of products formed (n) = 6 moles
Also given that, Pressure (P) = 2 atm
Temperature (T) = 819°C = (273 + 819)K = 1092 K
Gas constant, R = 0.08206 atm.L/mol.K
According to Ideal gas equation,
By substituting the above values in the equation,
The total volume of products formed when 128 g ammonium nitrite decomposed,
V = 268.8 L
Q3. (20 pts) Ammonium nitrite NH NO,, decomposes according to the following chemical equation NH,NO, (8)...
Q3. (20 pts) Ammonium nitrite NH.NO,, decomposes according to the following chemical equation. NH, NO, (s) → N, (g) + 2H,0 (g) What is the total volume of products obtained when 128 g NH NO, decomposes at 819 °C and 2.00 atm ? (Atomic weight of N=14.00 g/mol, H=1.01g/mol, O= 16.00 g/mol)
Q3. (20 pts) Ammonium nitrite NH.NO2, decomposes according to the following chemical equation. NH.NO, (s) → N, (g) + 2H,0 (g) What is the total volume of products obtained when 128 g NH.NO, decomposes at 819 °C and 2.00 atm ? (Atomic weight of N=14.00 g/mol, H=1.01g/mol, O= 16.00 g/mol)
Q3. (20 pts) Ammonium nitrite NH.NO2, decomposes according to the following chemical equation. NH,NO, (s) → N, (g) + 2H,0 (g) What is the total volume of products obtained when 128 g NH, NO, decomposes at 819 °C and 2.00 atm ? (Atomic weight of N=14.00 g/mol, H=1.01g/mol, O= 16.00 g/mol)
What is the total volume of products obtained when 128 g NH4NO2 decomposes at 819 o C and 2.00 atm NH4NO2 (s) → N2 (g) + 2H2O (g)
Ammonium nitrite, NH4NO2, decomposes upon heating to form N2 gas according to the following balanced chemical equation. When a sample of NH4NO2 was decomposed in a test tube, 813.9 mL of N2 gas was collected over water at 47.64 °C and the total pressure was 765.9 torr. NH4NO2(s) → N2(g) + 2 H2O(l). How many grams of N2 were collected?
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