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A silver block, initially at 56.2Celcius, is submerged into 100.0g of water at 25.2Celcius, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.5Celcius. What is the mass of the silver block?
How do I determine how much energy is needed to move an electron from n1 to n2 and n3? What is the formula
We find that 61.1 mL of an HCl solutionreacts exactly with 74.2 mL of 1.371 M KOH solution. Calculate the molarity of the HCl solution.
In a precipitate lab, if the step for digesting the precipitate were omitted, what would be the probable consequence of reporting the "percent limiting reactant" in the salt mixture? Explain.
2NH4NO3(s) delta--->2N2(g)+4H2O(g)+O2(g): a) How many liters of water vapor are produced when 25.8 g of NH4NO3 decomposes? b) How many grams of NH4NO3 are needed to produce 10.0 L of oxygen
If a 25.0 mL sample of sulfuric acid is titrated with 50.0 mL of 0.200 M potassium hydroxide to a phenolphthalein endpoint, what is the molarity of the acid? H2SO4(aq) + 2 KOH(aq) ? K2SO4(aq) + 2 H2O(l) Answer 0.300 M 0.200 M 0.150 M 0.400 M 0.100..
A solution of a dye was analyzed by spectrophotometry, and the following calibration data were collected. Dye Conc.(Y) (M) Absorbance(X) at 475 nm
If E(ethanol) and E(octane) are the energies per gram of fuel produced by ethanol and octane, respectively, calculations show that E(octane)/E(ethanol) is? [the standard molar enthalpy of formation of octane is -249.9 kJ/mol]
The nitrate ion (NO3-) is a very poor nucleophile. In fact, solvents such as water or methanol (also weak nucleophiles) are more reactive nucleophiles than the nitrate ion
fe 2hcl fecl2 h2 a piece of metallic iron 10 moles was dissolved in concentrated hydrochloric acid. the reaction
A sample of nitrogen gas at a pressure of 698 mm Hg and a temperature of 86oC, occupies a volume of 14.4 liters. If the gas is heated at constant pressure to a temperature of 116 oC, what the volume of the gas sample will be in L.
The following equilibrium is established: 1 H2O(g) + 1 CH4(g) ? 1 CO(g) + 3 H2(g) At equilibrium 0.03264 mol of CH4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = . Peq(CH4) = ..
For each reaction below, (a) identify the oxidation states of the atoms and (b) identify the oxidant, reductant, species oxidized, and species reduced. Also, think about this
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