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0.2500 g of zinc reacts with 50.00 mL of 0.1000 M hydrochloric acid to yield hydrogen gas. (a) Identify the limiting reagent and calculate the theoretical yield of hydrogen gas in mols. (b) If the hydrogen produced in (a) is collected over water, calculate the total volume of hydrogen gas which would be collected at 760 mm Hg and 25 degrees celsius. (Hint: Will a second gas be present in the sample collected by water displacement?)
A half-cell, made by dipping a silver wire into 0.05 M aqueous AgNO, at 298 OK, develops a half-cell potential of +0.740 volts. What is the standard half-cell (Eo) for silver?
Potassium nitrate has a lattice energy of -163.8 kcal/mo land a heat of hydration of -155.5 kcal/ mol. How much potassium nitrate has to dissolve in water to absorb
What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that is buffered at a pH of 4.55 and has a freezing point of -2.0 °C.
If 3.00 g of PbO2 was allowed to react with 2.00 g of Pb and 2.00 g of sulfuric acid, then 0.0116 mol of PbSO4 was obtained. What was the percent yield of PbSO4 (by weight) for this reaction?
1-phenyl-3-p-hydroxyphenyl-2-propen-1-one has a lower pKa value than does phenol. Account for this and the color of the phenoxide in terms of resonance structures for the anion.
A fertilizer manufacturing plant that produces 1,500 tons per day of fertilizer is known to emit particulate matter (PM) at a rate of 22 grams per ton of fertilizer produced.
Consider the unbalanced equation: C5H12(l) +O2(g) --> CO2(g) +H2O(l) if 25.2 grams of pentane (C5H12) are burned in excess oxygen, how many grams of H2O will be produced?
What are the molality and mole fraction of solute in a 29.3 percent by mass aqueous solution of formic acid (CH3OH)?
a solution containing 0.5000 moles of acetic acid per liter to 400.0 mL of 0.3000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77*10-5.
Determine the adiabatic flame temperature (C). Assume product temperatures of 1500K and 3000K, and then linearly interpolate.
Find the lowest temperature of vaporization and the highest temperature when there is liquid left over and Determine the range of temperatures which could be used for this process.
Consider the following first-order reaction: Reactant Product. This reaction has a half-life of 28.2 seconds. Calculate the rate constant.
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