Suppose a student repeats Experiment 1 using strontium instead of magnesium. The student adds 5.55 g of strontium to a crucible, heats the crucible and its contents for several minutes over a Bunsen burner, and records the final mass of the crucible and its contents. Write the balanced chemical equation for this reaction. Include physical states. balanced equation: What mass of product is expected to form in this reaction? Assume all of the strontium reacts. mass of product: 6.0 g

A 15.12 gram sample of iron is heated in the presence of excess sulfur. A metal sulfide is formed with a mass of 28.15g. Determine the empirical formula of the metal sulfide. Enter the elements in the order Fe,S empirical formula= ?  B) the References to access important values if needed for this question. A 22.60 gram sample of copper is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of29.35 g. Determine the empirical formula of the metal fluoride. Enter the elements in the order Cu,F empirical formula= ?

7.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 78. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 23.70g water 4.85g Use this information to find the molecular formula of X.

According to the law of conservation of mass, what mass of sodium metal is required to react with 0.355 g of chlorine gas to produce 0.585g of sodium chloride? A) 0.230 g B) 0.940 g C) 0.355 g D) 0.125 g E) impossible to predict from the given information

A sample of an oxide of vanadium weighing 4.589g was reduced with hydrogen gas to form water and another oxide of vanadium weighing 3.782g.The second oxide was reduced with hydrogen gas until only 2.573g of vanadium metal remained. a) Calculate the empirical formulas of the two oxides

If 2.952 g of copper(II) nitrate is reacted with sufficient sodium hydroxide, how much copper (II) hydroxide will be produced?

A 0.050 g sample of aluminum reacts with excess HCl.  How many moles of H2 can be produced?  Molar mass of Al = 26.982 g/mol

Write a balanced chemical equation based on the following description: solid cesium reacts with solid cesium nitrite to form cesium oxide and nitrogen gas.

suppose 1.57 g of Ca is heated in the air. what is the theoretical amount of CaO that will be produced?

What is the maximum mass of ammonia that can be produced from a mixture of 1.40 x 10' g N, and 4.60 x 10 g H2? Mass %3!