Question

nitrogen monoxide gas, which is used to treat some pulmonary diseases, is transported in pressurized gas cylinders. nitrogen monoxide gas is produced by reacting ammonia gas and oxygen gas, as represented by the following equation. equation i: 4nh₃(g) + 5o₂(g) → 4no(g) + 6h₂o(g) under high pressure in the gas cylinder, nitrogen monoxide gas can undergo the reaction represented by the following equation. equation ii: 3no(g) → n₂o(g) + no₂(g) the oxidation number for nitrogen in nh₃(g) is +/– (record in the first column) no(g) is +/– (record in the second column) n₂o(g) is +/– (record in the third column) no₂(g) is +/– (record in the fourth column) record your answer in the numerical - response section on the answer sheet (record your answer with no space, no sign and no comma in between numbers)

Explanation:

Step1: Determine oxidation number in NH₃

In NH₃, hydrogen has an oxidation number of + 1. Let the oxidation number of nitrogen be \(x\). Using the rule that the sum of oxidation numbers in a neutral compound is 0, we have \(x+(+1)\times3 = 0\). Solving for \(x\) gives \(x=- 3\).

Step2: Determine oxidation number in NO

In NO, oxygen has an oxidation number of - 2. Let the oxidation number of nitrogen be \(y\). Since the compound is neutral, \(y+( - 2)=0\), so \(y = + 2\).

Step3: Determine oxidation number in N₂O

In N₂O, oxygen has an oxidation number of - 2. Let the oxidation number of nitrogen be \(z\). For the neutral compound, \(2z+( - 2)=0\), solving for \(z\) gives \(z = + 1\).

Step4: Determine oxidation number in NO₂

In NO₂, oxygen has an oxidation number of - 2. Let the oxidation number of nitrogen be \(w\). Since the compound is neutral, \(w+( - 2)\times2=0\), so \(w=+4\).

Answer:

-3, +2, +1, +4