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5.50 moles of an ideal gas are expanded from 400 K and an initial pressure of 5.00 bar to a final pressure of 1.00 bar, and CP,m = 5/2R. Calculate w for the following two cases:
a) The expansion is isothermal and reversible.
b) The expansion is adiabatic and reversible.
c.) Calculate P,V and T for initial and final states of each process and produce a plot of the two processes on a P,V diagram. Without resorting to equations, explain why the result for part (b) is greater than or less than the result for part (a).
a buffer solution was made to have 1.4M HF and 1.10 M NaF. If .1 moles of NaOH are added to 1.00 L of the buffer, what will be the pH? Assume the volume remains constant. Ka of HF = 7.2E-4.
If 25 mL of 0.060 M HClO4 is mixed with 50 mL of 0.060 M KOH, what will be the resulting pH?
The element lithium has two naturally occurring isotopes, 7Li (isotopic mass 7.0160 amu, abundance 92.5 %) and 6Li (isotopic mass 6.0151 amu, abundance 7.50 %). Calculate the atomic mass of lithium.
24.6g of a hydrated salt of MgSO4.XH20, gives 12.0g of anhydrous MgSO4 on heating. What is the value of x?
How many double bonds are present in the "best" resonance structure of the phosphate ion?
What colligative properties are displayed by these situations.
How much energy (heat) is released when 1.9 moles of H2 reacts with 0.7 moles of Cl2 to create HCl(g) if the ΔHrxn = -184.6 kJ.
If the mass of the ore from which the gold was extracted is 166.0 g, what percentage of the ore is gold.
What is the principle quantum number for the inner transition metals? (the atomic numbers are 57 through 102, called the lanthanide series
Which statement is true concerning the reaction... N(g) + N(g) = N2(g) + energy?
If the presure of 50.0 mL of oxygen gas at 100oC increases from 735 mm Hg to 925 mm Hg, what is the final volume? Assume the temperature remains constant.
Assuming that its molar heat of vaporization is constant at 28.4 kJ/mol, the boiling point of C2H5NH2 when the external pressure is 0.709 atm is K.
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