To answer question 1, we observe that the volume of gas increased when the syringe was submerged in hot water and decreased when submerged in cold water. This is because gases expand when heated and contract when cooled. Temperature is a measure of the average kinetic energy of the gas particles. When the gas is heated, the particles move faster and collide with the walls of the syringe more frequently, causing an increase in pressure and volume. Conversely, when the gas is cooled, the particles move slower, collide less frequently, leading to a decrease in pressure and volume.
To answer question 2, we can assume that pressure is held constant in the experiment because the syringe is completely sealed, preventing any gas from escaping or entering. This means that the number of gas particles remains constant, and therefore the pressure remains constant.
To answer question 3, we can draw a straight line of best fit through the data points because the relationship between temperature and volume is expected to be linear due to the ideal gas law. The ideal gas law states that the volume of a gas is directly proportional to its temperature, assuming constant pressure and amount of gas. The straight line represents the linear relationship between temperature and volume.
To answer question 4, we need to extrapolate the line until it intersects the (negative) x-axis. The x-axis represents the temperature axis, and the y-axis represents the volume axis. When the line intersects the x-axis, it indicates a temperature of 0 K (-273°C). At this temperature, the volume of the gas would theoretically be zero, as the gas particles would have minimal kinetic energy and would occupy no space. However, in reality, reaching absolute zero is not achievable, so this intersection point is a theoretical extrapolation. The corresponding volume at this temperature can be estimated by reading the y-axis value at the intersection point.