Coupon Accepted Successfully!

General Chemistry

Open Flashcards


1 out of 13

Consider the reaction between nitric oxide and oxygen to form nitrogen dioxide. If 4 liters of nitrogen dioxide were formed, how many liters of nitric oxide and oxygen must have reacted?

A 2 L of NO & 1 L of O2
B 2 L of NO & 2 L of O2
C 4 L of NO & 2 L of O2
D 2 L of NO & 4 L of O2
Ans. C First, we should write the balanced equation. Without the balanced equation there is a good chance we might choose the incorrect answer.

According to the balanced equation, 2 liters of NO react with 1 liter of O2 to give 2 liters of NO2. According to the question, 4 liters of NO2 were formed. By taking proportionality, we can say that 4 liters of NO and 2 liters of O2 must have reacted so far.

Gases Flashcard List

13 flashcards
The behavior of gases can be predicted to a large extent on the basis of various laws. Gases are expressed mainly in terms of pressure, volume, and temperature. Many gases obey the ideal gas laws and those gases are called ideal gases. If we are not doing precision experiments, we can normally ignore the slight deviations that occur under normal conditions. Nevertheless, we cannot completely ignore the deviation factors. According to Boyle's law, the pressure is inversely proportional to the volume at a constant temperature. Charles' law states that the volume is directly proportional to the temperature at a constant pressure. Combining these laws and Avogadro's law gives the combined gas law. PV = nRT (The ideal gas law) Not all gases behave ideally. There are often deviations from the ideal behavior. At low temperatures, gases often behave differently apart from what is described by kinetic-molecular theory of gases. Considering these correction factors, the modified gas equation is: The correction constants or Vander Waal constants, a and b, of gases are experimentally found. The Van der Waal constants of some gases are given in Table 1. Table 1 Based on kinetic-molecular theory, which of the following are true? I. At a given temperature, all gases have the same average kinetic energy. II. At a given temperature, different gases have different average velocities. III. The average kinetic energy is proportional to the absolute temperature.A I onlyB II onlyC I & III onlyD I, II & III