This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.
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5.1 The graph shows a direct proportionality between pressure (P) and the inverse of volume ((1)/(V)). This relationship is described by Boyle's Law. Boyle's Law 5.2 An investigative question for this experiment could be: "How does the pressure of a gas change as its volume is varied, while keeping the temperature and amount of gas constant?" 5.3 The two variables that must be kept constant during the experiment to verify Boyle's Law are: • The temperature of the gas. • The amount (number of moles) of the gas. 5.4 Step 1: Locate the pressure value on the y-axis. From the graph, when the pressure is 200 kPa, find the corresponding value on the x-axis. Step 2: Read the inverse of volume from the graph. At P = 200 kPa, the value on the x-axis is 5 × 10^-2 cm^-3. So, (1)/(volume) = 5 × 10^-2 cm^-3. Step 3: Calculate the volume. Volume = (1)/(5 × 10^-2) cm^-3 = (1)/(0.05 cm)^-3 = 20 cm^3 The volume occupied by the gas is 20 cm^3. 5.5 Step 1: Calculate the inverse of the given volume. Given volume V = 11.11 cm^3. (1)/(V) = (1)/(11.11 cm)^3 ≈ 0.090009 cm^-3 Step 2: Determine the constant of proportionality (slope) from the graph. The graph is a straight line passing through the origin. Using the point (5 × 10^-2 cm^-3, 200 kPa): P = k ((1)/(V)) k = (P)/(1/V) = 200 kPa5 × 10^-2 cm^-3 = (200)/(0.05) kPa · cm^3 = 4000 kPa · cm^3 Step 3: Calculate the pressure using the constant k. P = k ((1)/(V)) = 4000 kPa · cm^3 × 0.090009 cm^-3 P ≈ 360.036 kPa The pressure exerted by the gas is approximately 360 kPa. 5.6 Two properties of an Ideal Gas are: • The particles of an ideal gas have negligible volume. • There are no intermolecular forces of attraction or repulsion between the particles of an ideal gas. Drop the next question.