Q3. (20 pts) Ammonium nitrite NH.NO2, decomposes according to the following chemical equation. NH,NO, (s) →...
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 NO,, decomposes according to the following chemical equation NH,NO, (8) ► N, (g) + 2H2O(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)
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?
UL Jyll 2) When ammonium nitrite (NH4NO2) is heated, it decomposes to give nitro This property is used to inflate tennis balls. a) Write a balanced equation for the reaction. (2 points) b) What is the partial pressure of N2 if a sample of 25.0 g NH4NO2 was heated at 100 °C in a 10.0 L reaction vessel until all the NH4NO2 had decomposed? (3 points) Calculate the quantity in grams y in grams of NH NO2 needed to inflate...
Consider the reaction of ammonium ions (NH and nitrite ions (NO2), shown in Equation 1. NH (aq) +NO2 (aq)N2 (g +2H O 0) Solutions of NH4 and NO2 were mixed in various quantities and the following rate data were obtained at a constant temperature: Experiment Initial [NH4 Initial [NO2] Initial rate for formation of N2 moVL s 3.04 x 10 6.08 x 10 1.22 x 10 0.1507.50 x 10 0.1501.50 102 0.300 1.50x 10 1. Find the order of the...
Ammonium carbonate decomposes upon heating according to the following balanced equation: (NH4)2CO3(s)→2NH3(g)+CO2(g)+H2O(g) Calculate the total volume of gas produced at 24.0 ∘C and 1.01 atm by the complete decomposition of 11.8 g of ammonium carbonate.
Enter your answer in the provided box. Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp =0.11 at 250°C NH HS(s) H2S() +NH3() If 60.5 g of NH HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium? PN atm Enter your answer in the provided box. Even at high temperatures, the formation of NO is not favored: (K-4.10x 10 at 2000°C) N28)+O2(g)= 2 NO(g) What is (NO] when a...
Ammonium nitrate decomposes explosively upon heating according to the following balanced equation: 2NH4NO3(s)→2N2(g)+O2(g)+4H2O(g) Calculate the total volume of gas (at 122 ∘C and 730 mmHg ) produced by the complete decomposition of 1.37 kg of ammonium nitrate.
Ammonium nitrate decomposes explosively upon heating according to the following balanced equation: 2NH4NO3(s)→2N2(g)+O2(g)+4H2O(g) Calculate the total volume of gas (at 119 ∘C and 761 mmHg ) produced by the complete decomposition of 1.71 kg of ammonium nitrate.