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A mixture consisting of 50 grams of ethanol and 50 grams of water is distilled using an efficient column. How much water will remain in the distillation flask the instant all of the azeotrope has distilled?
The pressure is steeply increased to 100 bar. The volume of the liquid is decreased by 1 ml at this constant pressure. Find the deltaH and deltaU
0.01M HCl reacts with 3.18 g Na2CO3. Here 50 mL of HCl is required for the reaction. Calculate the volume of CO2 produced at 273 K and 1 atm.
A 45.0-L steel tank at 20.0°C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many grams of acetylene are in the tank?
Calculate the mass of KI in grams required to prepare 4.00 102 mL of a 2.80 M solution.
which of the following accounts for the unusually high boiling point of water? the density of water, the hydrogen bonds in water
If 323 g of magnesium reacts with excess oxygen to produce 296 g of magnesium oxide, what is the percent yield for the reaction?
The peak was assigned as a Mn-Cl stretching mode of a contaminate manganese chloride species. Why would you expect this to be an erroneous assignment? Suggest a more likely source of this IR absorption.
Considering given equation as P4(s) + 5 O2(g) P4O10(s) where ΔH = -3013 kJ/mol you just need to compute the heat evolved when 436 grams of white Phosphorous (P4)burns in air according to the given equation as above.
What is the activation energy in kJ/mol? What is the rate constant at 100 degrees C?
A man has 50 kg of lipids and eats 1 kg of fish a day, which contains 0.5 ppm of methylmercury. What concentration of methylmercury will his lipids achieve?
Consider the dissolution of CaCl2. CaCl2(s) Ca2+(aq) + 2 Cl-(aq) ΔH = -81.5 kJ A 13.2 g sample of CaCl2 is dissolved in 106 g of water, with both substances at 25.0°C.
A 3.50-g sample of magnesium hydroxide was treated with 50.0 mL of a 0.500 M aqueous sulfuric acid solution. Calculate the number of grams of magnesium hydroxide that remained undissolved.
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