Question

Sort the nitrogen oxides listed below according to their percent by mass of oxygen. Nitrogen Oxides (6 items) (Drag and drop into the appropriate area below) N.O. NO N202 NO NO NO %O by Mass 50% or Less o More than SOKO Drag and drop here Drag and drop here Part 2 (2.5 points) Which two nitrogen oxides listed have unique empirical formulas compared to the others? Choose one or more: N20 ON2O3 N202 N204 O NO2 Ο NO

Answer 1

The nitrogen oxides are listed in order of their percent by mass of oxygen, and N₂O and NO₂ have unique empirical formulas compared to the others.

Step-by-step explanation:

The nitrogen oxides listed in order of their percent by mass of oxygen, from lowest to highest, are:

1. N.O. - 50% or less
2. N₂O - more than 50% but less than 100%
3. NO - 100%
4. N₂O4 - more than 100% but less than 200%
5. N₂O5 - more than 200%
6. NO₂ - more than 200%

The two nitrogen oxides that have unique empirical formulas compared to the others are N₂O and NO₂.

Answer 2

To sort the nitrogen oxides by percent mass of oxygen, calculate the mass percent for each compound (NO, NO₂, N₂O, N₂O₄, N₂O₅) and arrange them accordingly. Nitrous oxide (N₂O) and nitrogen monoxide (NO) have unique empirical formulas different from the other nitrogen oxides.

Step-by-step explanation:

To sort the nitrogen oxides by their percent by mass of oxygen, we need to calculate the percent composition of oxygen in each of the compounds. The formulas given are: NO, NO₂, N₂O, N₂O₄, N₂O₅. Using the data provided for molar masses, we calculate the mass ratios of O:N and then convert these to percentages. The mass of oxygen in each compound is obtained by multiplying the number of oxygen atoms by the atomic mass of oxygen (16 g/mol), and similarly for nitrogen (14 g/mol for each nitrogen atom).

For NO (molar mass = 14+16=30 g/mol), the percent by mass of oxygen is (16/30) × 100% = 53.33%.

For NO₂ (molar mass = 14+32=46 g/mol), the mass percent of oxygen is (32/46) × 100% = 69.57%.

For N₂O (molar mass = 28+16=44 g/mol), the mass percent of oxygen is (16/44) × 100% = 36.36%.

For N₂O₄ (molar mass = 28+64=92 g/mol), the mass percent of oxygen is (64/92) × 100% = 69.57%.

For N₂O₅ (molar mass = 28+80=108 g/mol), the mass percent of oxygen is (80/108) × 100% = 74.07%.

Now we can sort these values: N₂O < NO < NO₂ = N₂O₄ < N₂O₅.

For the second part of the question, the two nitrogen oxides with unique empirical formulas are N₂O and NO. This is because N₂O has a different ratio of nitrogen to oxygen atoms compared to the other oxides, which conform more to the general formula NOx.