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A 75.0 g sample of a pure liquid, liquid A, with a density of 3.00 g/mL is mixed with a 50.0 mL sample of a pure liquid, liquid B with a density of 2.00 g/mL. What is the total volume of the mixture? (Assume there is no reaction upon the mixing of A and B and volumes are additive)
Write down the balanced chemical equation when Fe 3 O 4 reacted with carbon monoxide and calculate mass of carbon dioxide that will be produced in this reaction if 234 g carbon monoxide is reacted with excess Fe 3 O 4 ?
When 10.0 g of NH3 reacts, the actual yield of N2 is 8.50 g. What is the percent yield?
what will happen if a small amount of HCl is added to a 0.1M solution of HF? a. the percent ionization of HF will decrease. b. Ka for HF will increase
Determine the total number of atoms in this chemical formula and calculate the molar mass of the solute and how many moles of solute are in the solution?
Pyridine(C5H5N) is a weaker base in H2O than 2,6 lutidine (dimethylpyridine), but we observe that the pyridine-BF3 complex is more stable than the comparable lutidine-BF3. Explain the reason for this inversion in stabilities.
Balance the following equation in basic solution. indicate which reactant becomes oxidized during the reaction, which reactant becomes reduced
When CuCN is used in the Sandmeyer reaction, the preparation is generally carried out in a neutral medium. Can you offer an explanation of why this is done?
KCL,KCLO3, and MnO2 having a total wight of 23.584 was jeated tp decompose the KCLO3. After heating, the mass was found to be 22.347g. how many moles of oxygen gas was evolved.
a .350 g sample of a biomolecule was dissolved in 15.0 g of chloroform, and the freezing point depression was determined to be .240 degree celcius. Calculate the molar mass of the biomolecule.
Calculate the heat released (kJ) in the reaction of 2.20 g of sulfur dioxide gas and excess oxygen gas to form sulfur trioxide gas
Determine the percent yield for the reaction between 3.74g of Na and excess O2 if 5.35g of Na2O2 is recovered
A sample of 255mg of neon occupies 3.00dm3 at 122K. Use the perfect gas law to calculate the pressure of the gas.
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