Consider the unbalanced equation: MgCl2(aq) + AgNO3(aq) AgCl(s) + Mg(NOJ2(aq) → a) If 5.00 g MgCl2 and 5.00 g AgNOs are allowed to react, how many grams of AgCl would be produced? b) Which reactant is not totally consumed by the reaction? How much remains (g)?

What is the approximate vapor pressure when the gas condenses at 70 degrees celsius

Find the mass, in grams, of 5.00*10^23 molecules of f2

There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. in the first step, calcium carbide and water react to form acetylene and calcium hydroxide: cac2 (s) + 2h2o (g) → c2h2 (g) + caoh2 (s) =δh−414.kj in the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6c2h2 (g) + 3co2 (g) + 4h2o (g) → 5ch2chco2h (g) =δh132.kj calculate the net change in enthalpy for the formation of one mole of acrylic acid from calcium carbide, water and carbon dioxide from these reactions. round your answer to the nearest kj .