Question

. which of the following statements about the combined gas law is incorrect? (a) at constant temperature the volume occupied by a definite mass of a gas varies inversely with the applied pressure. (b) doubling the volume and pressure of a sample of gas quadruples the absolute temperature. (c) at constant pressure the volume occupied by a definite mass of a gas varies inversely with the absolute temperature. (d) halving the volume of a sample of gas while doubling the pressure leaves the absolute temperature unchanged. (e) doubling the volume and pressure of a sample of gas doubles the absolute temperature.

Answer 1

The incorrect statement about the combined gas law is (c) 'at constant pressure the volume occupied by a definite mass of a gas varies inversely with the absolute temperature.' This contradicts Charles's law, where volume and temperature are directly proportional at constant pressure.

Step-by-step explanation:

Regarding the question about which statement about the combined gas law is incorrect, the incorrect statement is (c) 'at constant pressure the volume occupied by a definite mass of a gas varies inversely with the absolute temperature.' This is incorrect because according to Charles's law, at constant pressure, the volume of a gas is directly proportional, not inversely, to its absolute temperature.

The correct relationships can be summarized as follows:

• At constant temperature, the volume of a gas is inversely proportional to its pressure (Boyle's law).
• At constant pressure, the volume of a gas is directly proportional to its absolute temperature (Charles's law).
• At constant volume, the pressure of a gas is directly proportional to its absolute temperature (Amontons's law or Gay-Lussac's law).