Question

A sample of the compound M2SO4 weighing 0.1571g reacts with barium chloride and yields 0.3194g BaSO4....

A sample of the compound M2SO4 weighing 0.1571g reacts with barium chloride and yields 0.3194g BaSO4. write the balance equation ? and determine the molar mass and the identity of the metal M ?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Part A... Barium can be analyzed by precipitating it as BaSO4 and weighing the precipitate. When...
Part A... Barium can be analyzed by precipitating it as BaSO4 and weighing the precipitate. When a 0.255 g sample of a barium compound was treated with excess H2SO4 8.90×10−2 g of BaSO4 formed. What is the percentage of barium in the compound? Part B.. What is the percentage of sodium in pure table salt? Report your answer as a pecenteage to three significant figures. Part C.. An impure sample of table salt that weighed 0.8791 g when dissolved in...
Magnesium sulfate reacts with barium chloride according to the following balanced equation. If 1.20 g of...
Magnesium sulfate reacts with barium chloride according to the following balanced equation. If 1.20 g of magnesium sulfate is allowed to react with 10.0 g of barium chloride in a water solution, what is the theoretical yield of barium sulfate? MgSO4(aq) + BaCl2(aq) → BaSO4(s) + MgCl2(aq)
Tungsten metal reacts with chlorine to form a compound (containing only W and Cl) used in...
Tungsten metal reacts with chlorine to form a compound (containing only W and Cl) used in the production of filaments in incandescent light bulbs. 3.6768 g of W is reacted with excess chlorine gas and produces 7.930 grams of the material. A. Determine the formula of the compound B. Name the compound C. Determine the molar mass of the compound D. Write a balanced equation for the formation of the compound from W and Cl2 gas E. Determine the amount...
A solid sample formed by barium chloride and potassium nitrate, weighing 600 mg is subjected to...
A solid sample formed by barium chloride and potassium nitrate, weighing 600 mg is subjected to reaction with sulfuric acid solution in excess during the addition of the acid, we observed the formation of a precipitate, filtered, the precipitate, which after washed and dried weighed 0.050 g. The solution resulting from filtration was added a few drops of dilute H2SO4 and there was no precipitate formation. The resulting solution was transferred to a 250 mL volumetric flask and completed to...
Question 10 chap 4 A sample of 0.7960 g of an unknown compound containing barium ions...
Question 10 chap 4 A sample of 0.7960 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.7651 g, what is the percent by mass of Ba in the original unknown compound?
A 2.60 g sample of titanium metal reacts with 7.71 g of chlorine gas to form...
A 2.60 g sample of titanium metal reacts with 7.71 g of chlorine gas to form a compound. a) Determine the empirical formula of the titanium chloride salt b) Calculate the percent by mass of titanium and chloride in the salt
A sample of a gaseous binary compound of sulfur and fluorine weighing 0.989 g is decomposed...
A sample of a gaseous binary compound of sulfur and fluorine weighing 0.989 g is decomposed to give 0.293 g of solid S. In a separate experiment, the molar mass of the compound is determined to be 108 g/mol. Determine the molecular formula of the compound. Enter S before F.
Suppose a student performs a similar experiment to determine the empirical formula of a barium chloride...
Suppose a student performs a similar experiment to determine the empirical formula of a barium chloride hydrate. Given the data collected in the table above, what is the formula of the hydrate? The molar mass of water is 18.015 g/mol and the molar mass of barium chloride is 208.23 g/mol. (2 points) mass of empty crucible 55.060 g mass of crucible and hydrate 57.083 g mass of crucible and anhydrous salt 56.434 g
A 2.25 gram sample of zinc metal reacts with 5.00 grams of hydrochloric acid to give...
A 2.25 gram sample of zinc metal reacts with 5.00 grams of hydrochloric acid to give zinc chloride and hydrogen gas according the blanced equation: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) Molar mass ZnCl2: 136.28 g/mol a. What is the limiting reactant? b. What mass of ZnCl2 can be formed? (This is called the theoretical yield.)
I'm doing a chemistry lab on gravimetric analysis of a group 1 metal carbonate compound... So...
I'm doing a chemistry lab on gravimetric analysis of a group 1 metal carbonate compound... So basically, we heated the unknown metal carbonate, and then mixed it with calcium chloride solution. Then, we dried and weighed these products and recorded their masses. I'm having trouble finding the final mass & identity of the precipitate, alongside its molar mass. My balanced chemical equation is: CaCl2 + X2CO3 (where X = unknown group 1 metal) --> CaCO3 + 2XCl The mass of...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT