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A solution is made by dissolving 25g of NaCl in enough water to make 1.00 L of solution. Assume that the density of the solution is 1.00 g/cm3. Calculate the mass percent, molarity, molality, and mole fraction of NaCl
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A sealed vessel contains a gaseous mixture of H2 and excess O2. The mixture is at 500 K and has a total pressure of 140 kPa. After all of the hydrogen is reacted, the total pressure of the system measured at the same tem ...
A student finds that the mass of an object is 6.62 kg. She is told that her measurement has an error of 12.3%. What is the true mass (in kg) of the object?
Magnesium metal(0.100 mol) and a volume of aqueous hydrochloric acid that contains0.500 mol of HCl are combined and react to completion. How manyliters of hydrogen gas, measured at STP, are produced? Mg(s) + 2HCl(aq) --- ...
Silver nitrate has the molecular formula AgNO3. In a 109.0 g sample of silver nitrate, how much of that mass (in g) is from the silver atoms?
1-Write balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of nickel(II) iodide and potassium c ...
What wavelength of light (nm) is required to eject an electron with a speed of 2.0 x 10 6 m/s from a metal with a threshold energy of 3.4 x 10 -18 J?
Use valence bond theory to explain the bonding in F2, HF, and ClBr. Sketch the overlap of the atomic orbitals involved in the bonds.
What is the molarity, to the hundredths place, of 5.0 g HPO3 in 300. mL of solution?
A chemist adds 190.0 mL of a 2.8*10^-6 mol/L mercury(I) chloride (Hg2Cl2) solution to reaction flask. Calculate the micromoles of mercury(I) chloride the chemist has added to the flask. Round your answer to 2 significant ...
2 H2S(g) + 3 O2(g) → 2 H2O(g) + 2 SO2(g) Using standard enthalpies of formation, calculate the standard enthalpy change for this reaction.
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