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Liquifying PropanePlease show all work for the final calculations and answers. Thanks!
1) Calculate the entropy change that occurs when 3.5 moles of an ideal gas expands from 1.75 L at 20 degress Celsius to 8.46 L at .54 atm. Explain your strategy for solving this before you start.
2) Pop is packaged under CO2 (g) slightly above atmospheric pressure to make it fizzy. Calculate the change in Gibbs-free energy for the liquid and air in the bottle of root beer when it is opened at room temperature and the pressure drops from 1.8 atm to 1.0 atm. The volume of the liquid is 12 oz (about 29 mL = 1 oz) and the volume of the air space above the liquid is 35 mL. State any assumptions you may make.
3) Propane is a gas at room temperature and is 1 atm; yet, we know that when we store it as a fuel at room temperature for our grills and stoves, it is in liquid state. How is this done? Calculate the conditions needed to liquify propane at room temperature given that deltaH vaporization = 19.0 kJ/mol at 231.1 K.
At 1000 deg. K, a sample of pure NO2 gas decomposes. 2NO2(g)f/r2NO(g) + O2(g) The equilibrium constant Kp is 158. analysis shows that the partial pressure of O2 is 0.14 atm at equilibrium.
A 0.0490 molal aqueous NaBr solution freezes at -0.173°C. What is its apparent percent dissociation in this solution? Kf = 1.86°C/m for water. NaBr -> Na+ + Br-
A particular compound contains, by mass, 41.4g carbon, 3.47g hydrogen, and 55.1g oxygen a 0.100 mol sample of this compound weights 11.60 g.
Give an acceptable name and identify the functional group; and
When ethane C2H6 rea cts with chlorine Cl2 the main product is C2H5Cl but other products containing Cl such as C2H4Cl2 are also obtained in small quantities.
A rigid tank contains 1.50 moles of an ideal gas. Determine the number of moles of gas that nust be withdrawn from the tank to lower the pressure of gas from 25atm to 35 atm.
Important information about Molar concentrations, Calculate the molar concentrations, I-, disulfur octaoxide, disulfur trioxide.
A beaker with 1.30×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M .
The density of benzene at 15C is 0.8787 g/mL. Calculate the mass of 0.1500 L of benzene at this temperature.
Discuss the importance of economics as it relates to pollution prevention. Supple at least two seperate examples to augment your discussion.
We have a 100mL 0.2M AgNO3 solution and a 100mL 0.2M CH3COONa solution. Please describe how to prepare a 35 mL mixture solution containing 60mM AgNO3 and 140mM CH3COONa?
A chemist found that a certain amount of a CFC gas required 186 seconds to effuse through a porous plug when the pressure was held constant.
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