22.4 l of a gas at a temperature of 0*c are at a pressure of 2.0 atm. how many moles of gas are contained in the sample?

The moles of gas are contained in the sample is 2 (two) moles

Explanation:

We will use the formula PV=nRT

R= Regnault constant

n=number of moles

We convert the temperature into Kelvin according to: 0°C= 273K. In this case, the temperature is 273L.

PV=nRT   2 atm x 22,4l = n 0,082 l atm/K mol  x 273K

n = 2 atm x 22,4l/0,082 l atm/K mol  x 273K= 2 moles

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.