Nitrogen dioxide, a major air pollutant, can be produced by the combustion of nitrogen oxide as shown.
2no + o2 > 2no2
in a plant, 1,500 kg of nitrogen oxide is consumed per day to produce 1,500 kg of nitrogen dioxide per day. what is the percent yield?
21.7%
32.6%
43.5%
65.2%

Answer is: the percent yield is 65.2%.

Balanced chemical reaction: 2NO + O₂ → 2NO₂.

m(NO) = 1500 kg; mass of nitrog oxide.

From balanced chemical reaction: n(NO) : n(NO₂) = 2 : 2 (1 : 1).

m(NO) : M(NO) = m(NO₂) : M(NO₂).

1500 kg : 30 g/mol = m(NO₂) : 46 g/mol.

m(NO₂) = 1500 kg · 46 g/mol ÷ 30 g/mol.

m(NO₂) = 2300 kg.

the percent yield = 1500 kg ÷ 2300 kg · 100%.

the percent yield = 65.21%.

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.