Calculate the density (in g/L) of xenon gas in a 1200 mL flask at 28 °C and 620 torr. (Xe is monatomic; molar mass 131.3 g/mol.)

A precipitate will form when an aqueous solution of lead(II) nitrate is added to an aqueous solution of

When solutions of barium nitrate and ammonium sulfate are mixed, a white precipitate forms. What is the balanced net ionic equation for the formation of the precipitate?

What volume, in liters, would 1.60 moles of R-134a gas occupy at 28.00 °C and 692 mm Hg? (Report to 3 significant figures. Note: the gas density given for reference is not needed.)

Given the following reactions, estimate the overall enthalpy change for the dissolution of solid sodium hydroxide in water: NaOH(s) → Na+(aq) + OH-(aq).  Na(s) + ½H2(g) + ½O2(g) → NaOH(s)      ∆H° = −427 kJ/mol  Na(s) + H2O(l) → Na+(aq) + OH-(aq) + ½H2(g)      ∆H° = −184 kJ/mol  2 H2(g) + O2(g) → 2 H2O(l)      ∆H° = −572 kJ/mol 

Using ∆H°f(glucose) = −1274.4 kJ/mol, ∆H°f(H2O, l) = −187.8 kJ/mol, and ∆H°f(CO2, g) = −412.9 kJ/mol, calculate ∆H°rxn for the combustion of glucose [C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l)]. 

Which of these compounds results in the strongest electrolyte solution when dissolved in water?

When 80.0 J of energy is absorbed by 0.50 mol of water, how much does the temperature rise? The specific heat of water is 4.184 J/g·K.

An automobile air conditioner uses liquid R-134a (normal boiling point −26 °C). Inside the cabin, the pressurized liquid is allowed to expand and evaporate into a gas. At the molecular level, why does this evaporation cool the cabin air? 

All of the following ionic compounds of the Ni(II) cation are insoluble EXCEPT (i.e., which anion forms a soluble compound with Ni(II)?)