Monday

May 2, 2016
Total # Posts: 9

**College Chemistry**

The equilibrium constant for the conversion of cis-stilbene to trans-stilbene is Kc = 24.0 at 200 C. If cis-stilbene is placed in an empty container at an initial concentration of 0.850 mol/L. What is the final concentration of trans-stilbene in the container at equilbrium? A ...
*October 27, 2010*

**College Chemistry**

The rate constant for decomposition of compound X was determined to be 1.0x10^-4 s-1 at 298 K and 1.0x10^-2 at 365 K. The activation energy for reaction is: I dont know if this is correct 8.314 x 10^-3 x 298x365 divided by 365 - 298 x In 1.0 x10^-2 divided by 1.0-4. This gives...
*October 27, 2010*

**College Chemistry**

Calculate the cell potential for the following Galvanic cell: Co(s) Co2+ (0.15 mol L-1, ag)Fe 2+ (0.68 mol L-1, ag)Fe(s) Given that the standard reduction potential Eo for Co2+ is -0.28 V and Eo for Fe2+ is -0.44 V. Anwer is -0.14 V The left side of the above equaton is the ...
*October 27, 2010*

**College Chemistry**

A Galvanic cell consists of Mg electrode in a 1.0 mol L -1 Mg(NO3)2 solution and a Ag electrode in a 1.0 mol L-1 AgNO3 solution. Calculate standard emf for the spontaneous reaction of this electrochemical cell at 25 C, given that the standard reduction potential Eo for Ag+ is...
*October 27, 2010*

**College Chemistry**

What is pH of the buffer 0.1 mol L-1 Na2HPO4/0.15 mol L-1 KH2PO4? (Given Ka(H2PO4-)=6.2x10 power-8). Sorry if the power is confusing. My computer does not have the symbol. Thanks
*October 22, 2010*

**College Chemistry**

What is pH of an aqueous solution formed by adding 20 mL of 0.1 mol L-1 NaOH to 30 mL of 0.2 mol L-1 HCI? Please show steps and maths. Is there a unit conversion if so how is this done. Thank you
*October 22, 2010*

**College Chemistry**

Calculate pH of a 1.0 mol L -1 boric acid solution. (Ka(H3BO3) = 5.8 x 10 power -10 Please solve this problem. My computer does not have the power symbol. Can you please show maths and steps. Is mollar mass required of the above. Is -log and constant above used. Thanks
*October 22, 2010*

**College Chemisty**

The pH of water collected in a stormwater run-off downstream from a Union Carbide chemical factory is 4.82. Calculate the H+ ion concentration of rainwater. The problem may start with: pH= -log H+ = 4.82. The answer is 1.5x10 power -5. Again, Can you please show steps for maths.
*October 22, 2010*

**College Chemistry**

A student weighs out 0.568 g of KHP (molar mass=204g/mol) and titrates to the equivalence point with (36.78 cm cubed which is 3) of a stock NaOH solution. What is concentration of stock NaOH solution? KHP is an acid with one acidic proton. The word cubed is in word form ...
*October 22, 2010*

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