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Determine the freezing point of an aqueous solution that is 1,7 m in ethylene glycol. The freezing point depression constant for water is 1.86°C/m The freezing point of pure water is 0.0°C.
a sample of oxygen that occupies 1.00X 10^6 ml at 575 mm hg is subjected to a pressure of 1.25 atm. what will the final volume of the sample be if the temperature is held constant?
If it takes 52 J of energy to warm 7.40g of water by 17°C, how much energy would be needed to warm 7.40g of water by 55 °C
The equilibrium constant is 100. Calculate the concentrations of O2 present at equilibrium
Calculate that how many grams of potassium chloride remain dissolved and how many grams came out of this given solution?
What is the first step in the reaction sequence of Aldol reactions under basic conditions? a. Removal of the aldehyde proton b. Removal of an alpha proton to form the enolate
A concentrated sulfuric acid solution is 74.0% H2SO4 by mass and has a density of 1.66 g/mL at 20°C. (MW of H2SO4 is 98.0 g/mol.) The molality of the H2SO4 solution is ?
A 335 mL container holds 0.146 g of Ne and an unknown amount of Ar at 35°C and a total pressure of 628 mmHg. Calculate the moles of Ar present.
mass of magnesium = .021 grams initial volume = 50.00 mL final volume = 25.6 volume of liquid displaced = 24.4 volume of hydrogen gas produced = 24.4?
what would the rate constant be at a temperature of 150C for the same reaction described in Part A?
The titration of 0.7910 grams of an unknown weak acid requires 41.5 mL of 0.139 M NaOH in order to reach the equivalence point.
calculate E when 830.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm.
A sample of nitrogen (9.27g) reacts completely with magnesium, according to the equation: 3 Mg + N2 -> Mg3N2. The mass of Mg consumed is ____g?
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