Gaseous state - student copy

NJC/2020/I/7 5 Which diagram correctly describes the behaviour of a fixed mass of an ideal gas? A B C D NYJC/2020/I/5 6 Which graph correctly describes the behaviour of two ideal gases P and Q , both having the same mass, where P has a larger M r than Q ? A B 0 T/ o C p / atm constant V 0 V/ cm 3 p / atm constant T T / o C p Q P T / o C p Q P 0 V/ cm 3 pV constant T 0 T/ o C V/ cm 3 constant P constant V constant V

RI/2020/III/1b 12 (b) An important property of an aerosol propellant is that it should be a gas at room temperature and pressure. (i) State two assumptions of the kinetic theory as applied to an ideal gas. [2] (ii) Fig. 1.1 illustrates the behaviour of 1 mol of ideal gas at 293 K. Fig. 1.1 On Fig.1.1, sketch and label the graph for 1 mol of N 2 O at 293 K. [1] (iii) On the same axes in Fig. 1.1, sketch and label the graph for 1 mol of N 2 O at 500 K. Explain your answer. [2] SAJC/2020/III/4a 13 Coronavirus disease 2019 (COVID-19) is an infectious disease that has spread globally. One of the most common symptoms developed by people affected with COVID-19 is difficulty in breathing. (a) During breathing, the lungs take in oxygen gas and remove carbon dioxide gas. During inhalation, the volume of the lungs increases, causing air to flow into the lungs. During exhalation, the volume of the lungs decreases, causing air to flow out of the lungs. 1 p ideal gas pV RT

YISHUN INNOVA JUNIOR COLLEGE 2021 JC2 H2 CHEMISTRY THE GASEOUS STATE (ADVANCED) DHS/2020/I/6 1 A container with a volume of 120 m 3 with an internal pressure of 1 bar at 320 K was joined to two containers as shown below. One of them has a volume of 12 m 3 with a vacuum within, while the other has a volume of 32 m 3 with an internal pressure of 2 bar and a temperature of 273 K. What is the final pressure, in bar, in the combined containers when the taps were opened and the temperature allowed to equilibrate to 298 K? A 0.23 B 0.38 C 1.11 D 1.20 120 m 3 1 bar 320 K 12 m 3 vacuum 32 m 3 2 bar 273 K taps

B 0.025 × 273 × 22.7 0.10 × 373 C 0.025 × 373 × 22.7 0.10 × 273 D 0.10 × 373 × 22.7 0.025 × 273 EJC/2020/III/3a 7 Henry’s law is a gas law that states that, at a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid, is directly proportional to the partial pressure of that gas, in equilibrium with that liquid. The proportionality factor is called Henry’s law constant. Suppose gaseous A is in equilibrium with a solution of A in water:     2 H O A g A aq sol H  The Henry’s law solubility constant, K H , of A in water, is given by     H A g A aq K p      where   A g p is the partial pressure of A in the gaseous phase   A aq     is the concentration of A, in mol dm – 3 , in the aqueous phase (a) Soda manufacturers often inject cold liquid with pressurised carbon dioxide, then can the drink under high pressure. On the average, a typical 355 cm 3 soda can possesses an internal pressure of 120 kPa when canned at 4 ºC, and 250 kPa when stored at room temperature. The Henry’s law constant, K H , of CO 2 in water is 3.4 × 10 – 7 mol dm – 3 Pa – 1 at room temperature. (i) Explain why the internal pressure is so much higher than what is predicted by the ideal gas equation when the temperature is raised during storage. [1] (ii) Calculate the concentration of CO 2 dissolved in a typical soda can at room temperature, in mol dm – 3 . [1] After opening a can of soda, the drink eventually goes flat when the dissolved CO 2 escapes into the atmosphere.