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1- verify that the 2s wavefunction for hydrogen is normalized.
2- use the wavefunction for the 1s orbital to find the expression value for r
calculate w and ?U when 1 mole of xenon gas assumed ideal under goes adiabatic expansion from 27?c to 127? assuming(heat capacity of constant volmue=12.5)
When 20.0 grams of an unknown compound are dissolved in 500. grams of benzene, the freezing point of the resulting solution is 3.77°C. The freezing point of pure benzene is 5.48°C, and Kf for benzene is 5.12°C/m. What is the molecular weight of th..
copper solid metal and copper sulfate, and of course a salt bridge filled with KCl. What voltage would you expect from this cell at room temperature and 1M ZnSO4 solution but 0.01M CuSO4 solution
Solutions of strontium hydroxide, silver nitrate, hydrogen phosphate, potassium nitrate, and copper (II) sulphate are prepared and placed in separate containers. Consider the reaction of the pairs of these compounds.
what volume of ethylene glycol, a nonelectrolyte, must be added to 15.0 Liters of water to produce an antifreeze solution with a freezing point of - 30 degrees celcius? what is the boiling point of the solution?
Dry ice is solid carbon dioxide. A 1.87g sample of dry ice is placed in an evacuated 4.03 L vessel at 22 degrees C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas
Show the bond angles which are at least slightly different that are shown by the H2CCBr2 molecule.
At 298, 1 atm, the heat produced by the reaction of 4.00mol of NO with molecular oxygen heats 1.07L liquid water from 298k to 348k. Calculate enthalpy for the reaction 2NO + O2 -> NO2, at 298k. Assume constant pressure and no heat lost.
Consider: C7H16 (l) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (l) ΔH°reaction=- 4130 kJ. How much energy is released when 4.000 moles of C7H16, is combusted?
An organic compound X contains C, H, and O. A 16.69 g sample of X underwent combustion analysis, leading to the production of 44.71 g CO2 and 10.99 g H2O. What is the emperical formula of the compound?
Ammonium Nitrate absorbs 3.30 x 10^2 J of heat per gram dissolved in water. In a coffee-cup Calorimeter, 4.40 G NH4NO3 is dissolved in 100 g of water at 21.0 degrees celsius. What is the final temperature of the solution
consider the reaction CO2+H2=CO+H2O.The equilibrium concentrations are [CO]= 0.050M, [H2]=0.045M, [CO2]=0.086M, and [H2O]= 0.040M. Calculate K .
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