Answer:
1. 0.14 g of NO2.
2. 0.27 g of CO2.
Explanation:
The balanced equation for the reaction is given below:
2C8H10N4O2 + 27O2 —> 16CO2 + 10H2O + 8NO2
Next, we shall determine the mass of caffeine, C8H10N4O2 that reacted and the masses of nitrogen (iv) oxide, NO2 and carbon (iv) oxide, CO2 produced from the balanced equation. This can be obtained as follow:
Molar mass of of C8H10N4O2 = 194.19 g/mol
Mass of C8H10N4O2 from the balanced equation = 2 × 194.19 = 388.38 g
Molar mass of CO2 = 44.01 g/mol
Mass of CO2 from the balanced equation = 16 × 44.01 = 704.16 g
Molar mass of NO2 = 46.01 g/mol
Mass of NO2 from the balanced equation = 8 × 46.01 = 368.08 g
Summary:
From the balanced equation above,
388.38 g of caffeine, C8H10N4O2 reacted to produce 704.16 g of CO2 and 368.08 g of NO2.
1. Determination of the mass of NO2 produced from the reaction.
This can be obtained as follow:
From the balanced equation above,
388.38 g of caffeine, C8H10N4O2 reacted to produce 368.08 g of NO2.
Therefore, 0.15 g of caffeine, C8H10N4O2, will react to produce = (0.15 × 368.08) / 388.38 = 0.14 g of NO2.
Therefore, 0.14 g of NO2 was obtained from the reaction.
2. Determination of the mass of CO2 produced from the reaction.
This can be obtained as follow:
From the balanced equation above,
388.38 g of caffeine, C8H10N4O2 reacted to produce 704.16 g of CO2.
Therefore, 0.15 g of caffeine, C8H10N4O2, will react to produce = (0.15 × 704.16) / 388.38 = 0.27 g of CO2.
Therefore, 0.27 g of CO2 was obtained from the reaction.
