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Consider the following table of thermodynamic data. All values are tabulated at 250C. Substance deltaGf0 (kJ/mol) deltaS0 (J/mol.K) C2H2 (g) 209 201 C2H4 (g) 68 219 C2H6 (g) - 33 230 H2 (g) 0 131 H2O (g) - 229 189 C2H5OH (l) - 175 161 What is the value of deltaH0 (in kJ) for the reaction described below? Assume the reaction is performed at 250C. C2H2 (g) + 2H2 (g) -----> C2H6 (g) a. - 248 b. - 311 c. - 173 d. 236
Chlorine forms a number of oxides with the following oxidation numbers: +1,+3,+4,+6 &+7.Write formula for each of these compounds.
What is the pH of a solution containing 50.00 mL of 1.0 M HCl and 50.00 mL of 1.0 NH3? The Kb for NH3 = 1.8 x 10-5.
A sample contained a mixture of CdS and ZnS. The amount of CdS was determined by reacting 5.903 g of the sample with an excess of HCl to release H2S from each compound
how do i prepare 50 mL of the 0.00625 M HCl solution by an appropriate dilution of the 0.0125 M HCl solution
which is the desired product, can decompose to product F, how might you ensure that you stopped the reaction at the optimum point to ensure the maximum yield of C?
An aerosol can has a gas pressure of 133 kPa at 293 K. Calculate the pressure when the can is heated to 460 K.
The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are..
what is the likely magnitude of the equilibrium constant K? Hydrogen is used as a rocket fuel because it is very light and reacts explosively and completely with oxygen. For the combustion reaction
Identify the limiting reagent and the volume of CO2 formed when 11L CS2 reacts with 18L O2 to produce CO2 gas and SO2 gas at STP.
In 13C NMR, splitting of spectral lines is due to: A) coupling between a carbon atom and protons attached to that carbon atom b) coupling between a carbon atom and protons attached to adjacent carbon atoms
suppose that a student performing an experiment mistakenly calibrated the pH meter using pH 6 instead of a pH 7 buffer. As a result all pH meter readings were too low.
Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the ammonium acetate is dissolved in it.
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