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Calculate the final temperature of solution when 12 g of oxalic acid, (COOH)2(s), is dissolved in 84 mL of water that is initially at 26 C. The enthalpies of formation of oxalic acid in the solid and aqueous phases are -826.8 and -818.8 kJ/mol, respectively. The heat capacity of water is 4.184 J/g*K. Ignore the heat capacity of oxalic acid.
calculate the initial reaction rate when [O3] & [NO] remain essentially constant at the values [O3]0= 7.48 x 10-6 M & [NO]0= 3.26 x 10-5M, owing to continuous production from separate sources.
How many milliliters of a stock solution of 2.00M KNO3 would you need to prepare 100.0 mL of 0.150M KNO3?
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.120 M HClO(aq) with 0.120 M KOH(aq). The ionization constant for HClO is 4.0×10-8
the diffusion coefficient for nitrogen in the metal at 1150 C is 1x10^-11 m^2/s and the end is 3.5 kg/m^3, what is the nitrogen concentration at a position 2mm into the sheet away from higher concentration end?
How much energy (in kilojoules) is required to convert 245 mL of diethyl ether at its boiling point from liquid to vapor if its density is 0.7138 g/mL ?
Derive the general expression for the work per kilomole of a van der waals gas in expanding reversibly and at a constant temperature
How many distinct terminal alkynes exist with molecular formula C5H8?
Determine the mass of propylene glycol neded to substitute one gallon of ethylene glycol and also find out the volume of propylene glycol, required to get the same antifreeze protection as one gallon of ethylene glycol.
A 10.00 ml sample of vinegar, density 1.01 g/ml was diluted to 100.00 ml volume. It waas found that 25.0 ml of the diluted vinegar required 24.15 ml of 0.0976 M NaOH to neutralize it
Compare the energy of a photon of wavelength 3.4 um with that of wavelength 0.155 nm. answer is in E1/E2
The specific heat of liquid water is 4.184 J/g x C. Calculate the energy required to heat 10.0 g of water from 26.5 C to 83.7 C.
Calculate the number of moles of quicklime, CaO, that would be produced by the decomposition of 30.0 moles of limestone, CaCO3, in the following reaction.
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