The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated. Find the mass of PH3 that forms from the reaction of 1.00 g NH3.

Ammonia reacts with O2 to form either NO(g) or NO2(g) according to these unbalanced equations: NH3(g) O2(g) ⟶NO(g) H2O(g) NH3(g) O2(g) ⟶NO2(g) H2O(g) In a certain experiment 2.00 moles of NH3(g) and 10.00 moles of O2(g) are contained in a closed flask. After the reaction is complete, 6.75 moles of O2(g) remains. Calculate the number of moles of NO(g) in the product mixture: Hint: You cannot do this problem by adding the balanced equations because you cannot assume that the two reactions w

SOLVED: The combustion of ammonia proceeds by the reaction:NH3(g) O2(g) → NO2(g) H2O(g)Oxygen pressure was measured over a specific time period and shown to decrease by 7.7 torr. What is the rate of production of NO2 over that same time period?9.7 mol/s2.0 torr/s44 torr/storr/s

SOLVED: The thermochemical equation showing the formation of ammonia(NH3) from its elements is:N2 (g) 3 H2 (g) —> 2 NH3(g) ΔH = -92 kJThis equation shows that 92 kJ of heat is:a. Lost to the surroundings when one mole of hydrogen is used upin the reaction.b. Absorbed from the surroundings when one mole of nitrogenreacts.c. Absorbed from the surroundings when one mole of ammonia isformed.d. Lost to the surroundings when 2 moles of ammonia isformed.

Nitrification | Definition, Process & Cycle