For the following reaction, 72.0 grams of barium chloride are allowed to react with 64.0 grams of potassium sulfate. barium chloride(aq) + potassium sulfate(aq) →→→→→barium sulfate(s) + potassium chloride (aq) What is the maximum amount of barium sulfate that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams

Barium carbonate is the source of barium compounds.  It is produced in an aqueous precipitation reaction from barium sulfide and sodium carbonate.  (Barium sulfide is a soluble compound obtained by heating the mineral barite, which is barium sulfate, with carbon.)  What are the molecular equation and net ionic equation for the precipitation reaction?  A solution containing 33.9 g barium sulfide requires 21.2 g of sodium carbonate to react completely with it, and 15.6 g of sodium sulfide is produced in addition to whatever barium carbonate is obtained.  How many grams of barium sulfide are required to produce 500 tons of barium carbonate?

What type of chemical reaction is illustrated in the following example?             N2(g) + H2(g) → NH3(g)   A) combination reaction B) decomposition reaction C) single-replacement reaction D) double-replacement reaction E) neutralization reaction    What type of chemical reaction is illustrated in the following example?             Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g)   A) combination reaction B) decomposition reaction C) single-replacement reaction D) double-replacement reaction E) neutralization reaction  What type of chemical reaction is illustrated in the following example?             AlCl3(aq) + AgNO3(aq) → Al(NO3)3(aq) + AgCl(s)   A) combination reaction B) decomposition reaction C) single-replacement reaction D) double-replacement reaction E) neutralization reaction

A 0.8910 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then treated with an excess of AgNO3 to yield 1.923 g of AgCl. Calculate the percent by mass of each compound in the mixture. Be sure each of your answer entries has the correct number of significant digits. % mass NaCl 0% % mass KCI X

In the laboratory, a student dilutes 25.3 mL of a 8.46 M hydrobromic acid solution to a total volume of 100.0 mL. What is the concentration of the diluted solution?

For the following reaction, 6.80 grams of water are mixed with excess chlorine gas. The reaction yields 15.1 grams of hydrochloric acid. chlorine (g) + water (1) →→→→hydrochloric acid (aq) + chloric acid (HCIO3) (aq) What is the theoretical yield of hydrochloric acid ? || What is the percent yield of hydrochloric acid ? grams %

In an experiment, a student combines 75.0 mL of a 0.190 M iron (III) chloride solution with 125.0 mL of a 0.240 M sodium carbonate solution. What is the theoretical yield of sodium chloride (in grams)?

In an experiment, a student combines 75.0 mL of a 0.200 M iron (III) chloride solution with 125.0 mL of a 0.250 M sodium carbonate solution. Write a balanced equation for the reaction. What is the limiting reactant? What is the theoretical yield of sodium chloride (in grams)? How many grams of sodium chloride need to be produced in the experiment in order to achieve a yield of 93.75%?

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 48.82 mL of the sodium hydroxide solution was required to react with 0.7540 g KHP. Calculate the molarity of the sodium hydroxide. Molarity = ___________ M

Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction.   NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g)  Balance the reaction.