When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of FeO and Fe2O3. In a certain experiment, 20.00 g of iron metal was reacted with 11.20 g of oxygen gas. After the experiment, the iron was totally consumed and 3.24 g of oxygen gas remained. Calculate the amounts of FeO and Fe2O3 formed in this experiment.
Answer to relevant QuestionsElement X forms both a dichloride (XCl2) and a tetra-chloride (XCl4). Treatment of 10.00 g of XCl2 with excess chlorine forms 12.55 g of XCl4. Calculate the atomic weight (mass) of X and identify X. When M2S3(s) is heated in air, it is converted to MO2(s). A 4.000- g sample of M2S3(s) shows a decrease in mass of 0.277 g when it is heated in air. What is the average atomic mass of M? A 2.077 g sample of an element, which has an atomic mass between 40 and 55, reacts with oxygen to form 3.708 g of an oxide. Determine the formula of the oxide and identify the element. Consider the following diagram. A porous container (A), filled with air at STP, is contained in a large enclosed container (B), which is flushed with H2(g). What will happen to the pressure inside container A? Explain your ...You have two samples of helium gas at the same pressure in separate steel containers of the same volume. You want the number of collisions of helium atoms with the walls of container 1 to be twice the number of collisions of ...
Post your question