An aqueous solution of HNO2 is poured onto a solid pile of SrCO3. Identify the net ionic equation for this reaction.

A) SrCO3(s) + 2 HNO2(aq) → Sr(NO2)2(aq) + HCO3(aq)
B) no reaction occurs
C) Sr2+ + CO32- + 2 H+ → Sr2+ + H2O + CO2(g)
D) SrCO3(s) + 2 HNO2(aq) → Sr(NO2)2 + H2O + CO2(g)
E) SrCO3(s) + 2 H+ → Sr2+ + H2O + CO2(g)

Which of the following elements would you expect to have the lowest ionization energy value? fluorine, lithium, neon, nitrogen

Using a value of ksp = 1.8 x 10-2 for the reaction pbcl2 pb+2(aq) + 2cl -(aq). if the value of ksp was determined to be only 1.2 x 10-2: too much solid has dissolved. additional precipitate is forming. the solution is unsaturated. the ions are now combining to reduce their concentrations.

Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4nh3 (g) + 5o2 (g) → 4no (g) + 6h2o (g) also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium nh3 65.1atm o2 31.3atm no 62.7atm h2o 65.8atm compound pressure at equilibrium nh3 65.3 atm o2 7.79 atm no 12.1 atm h2o 65.8 atm calculate the value of the equilibrium constant kp for this reaction. round your answer to 2 significant