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Phase Diagram for Methane
1. What are the approximate temperature and pressure at the critical
point?
2. What are the approximate temperature and pressure at the triple
point?
3. Is methane a solid, liquid, or gas at 1 atm and 0 ºC?
4. What phase(s) will exist at point 1?
5. If solid methane at 1 atm is heated while the pressure is held
constant, will it melt or sublime?
Based from the phase diagram of water and carbon dioxide, answer the following
questions and justify your answers:
1. You have ice at 263 K (-10.0 °C) and 1.0 atm. What could you do to make
the ice sublime?
2. A sample of dry ice (solid CO2) is cooled to 173 K (-100.0 °C), and is set
on a table at room temperature (298 K; 25 °C). At what temperature is the
rate of sublimation and deposition the same (assume that pressure is held
constant at 1 atm)?
Illustrate the phase diagram of a substance given with the following points: a
triple point at 0.70 atm and 80 ºC; a normal freezing point at 100 ºC; a normal
boiling point at 350 ºC; and a critical point at 1.6 atm and 810 ºC. For this,
complete the following:
1. Roughly sketch the phase diagram, using units of atmosphere and degree
Celsius. Label the area 1, 2, and 3, and points T and C on the diagram.
2. Describe what one would see at pressures and temperatures above 1.25 atm
and 300 ºC.
3. Describe the phase changes from 100 ºC to 200 ºC at 1.5 atm.
4. What exists in a system that is at 1 atm and 100 ºC?
5. What exists in a system that is at 1 atm and 325 ºC?
For How Long Must A Current Of 1.5 Ampere Be Passed Through An Aqueous Solution Of A Copper Salt During Electrolysis In Order To Deposit 2.50g Of Copper (cu=63.5)
Gold has a density of 19.3 g/cm3 and has a mass of 10 kg. What is the volume of the gold bar? Is it more or less dense than Silver that has a density of 10.5 g/cm³.(4)
Activity 4.1.1. Reaction time! Write the rate expressions for the following
reactions in terms of the disappearance of the reactants and the appearance
of the products:
1. (aq) +OCH(aq)
Cl(aq) + Ol'(aq)
Activity 4.1.1. Reaction time! Write the rate expressions for the following
reactions in terms of the disappearance of the reactants and the appearance
of the products:
1. (aq) +OCH(aq)
Cl(aq) + Ol'(aq)
Caculate the volume, in ml of 0.2 M NaOH solution that contains 6.0 g of NaOH.
35 grams of ethanol is dissolved in 115 grams of water. What is the concentration of ethanol in parts per billion (ppb)
A 4.00 L rigid vessel (see figure below) holds 2.00 L of pure water. The remaining volume holds N2 at 45.0°C. At this stage the pressure gauge on the vessel reads 85.0 kPa. You then load 13.2 g of Be(NO3)2(s) and 15.4 g of N2H5Cl(s) to the container. The salts dissociate completely and a reaction occurs producing both NO(g) and more N2(g). After the reaction has completed, the temperature increased by 5.00°C, with no change in the liquid volume.
Assume that:
o No gas escaped or entered the vessel during the loading of the reagents.
o The liquid phase is free of any gaseous species.
o The ideal gas law applies.
o The reaction is irreversible with a yield of 88.0%.
i. Show that the balanced reaction in alkaline (basic) medium is given by:
4𝑁𝑂3 − (𝑎q) + 3𝑁2𝐻5 + (𝑎q) → 4𝑁𝑂(𝑔) + 3𝑁2(𝑔) + 7𝐻2𝑂(l) + 𝑂𝐻(𝑎q) −
(Show all balancing steps clearly)
ii. Calculate the number of moles of N2(g) and NO(g) after the reaction.
iii. Calculate the partial pressure of N2(g) and NO(g) in kPa after the reaction
