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Calculate the partial pressure of O2 produced from 1.44 L of 0.508 M N2O5 solution at 45 degrees C over a period of 20.6 hours if the gas is collected in a 11.7 L - container. (Assume that the products do not dissolve in chloroform.)
Dinitrogen pentoxide decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 degrees C of 1.0 x 10^-5 s^-1.
Predict the products for the following set of reactants- PCl3(l) + H2O(l) ? (You are just asked to determine the products and not necessarily balance the equation)
A standard Ni(s) |Ni^2+ (aq) || Ag^+ (aq) | Ag(s) is constructed and the standard potential is 1.03 V a) write a balanced reaction for the cell
Consider the conversion of CH3CH2CH2CH2OH to each of the compounds shown below. In which conversion is an oxidizing agent required
Some of the original solid remained and total pressure in container was 7.76 atms when equilibrium is reached. Calculate number of moles of H2O(g) present at equilibrium How many grams of original solid remain
Calculate the percentage of acetic acid that exists in ionized form when dissolved in water at 0.5 M total concentration.
How many valence electrons are there for the POCl3 molecule? Draw a reasonable Lewis structure for POCl3. Assign formal charges for the atoms in your Lewis structure. Draw a second legitimate resonance contributor for POCl3. Assign formal charges ..
How many milliliters of 0.200 M NaOH will be required to titrate 19.6 mL of 0.479 M H2SO4
Calculate the enthalpy change per mole for this process. ( Assuming C=4.18 J deg c^-1 g^-1 and density of the final solution is 1.00g/ml).
The molar mass of corn oil is 890g/mole. How many moles and how many grams of sodium hydroxide are required to react with the 15mL (13.7g) of corn oil? Show your calculations.
Compute the expected change in temperature for 1.7 grams of ammonium nitrate NH 4 NO 3 dissolved in 50.0 mili litres of water H 2 O.
which of these is true about the following reaction?
2 NH3(g) + 3 O2(g) + 2 CH4(g) → 2 HCN(g) + 6 H2O(g) If 5.08 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be produced, assuming 100% yield?
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