A 1.500 g piece of calcium metal reacts with oxygen gas to form 2.099 g of calcium oxide. Calculate the empirical formula of calcium oxide
A 1.500 g piece of calcium metal reacts with oxygen gas to form 2.099 g of...
1. A 0.750-g sample of tin metal reacts with 0.201 g of oxygen gas to form tin oxide. Calculate the empirical formula of the tin oxide. 2. A 0.565-g sample of cobalt metal reacts with excess sulfur to give 1.027 g of cobalt sulfide. Calculate the empirical formula of the product. 3. A 1.164-g sample of iron filings reacts with chlorine gas to give 3.384 g of iron chloride. Calculate the empirical formula of the product? 4. A 0.626-8 sample of copper oxide...
When 4.20 g of calcium metal reacts with 2.80 g oxygen gas, 5.12 g of calcium oxide is produced. What is the percent yield of the reaction?
7. A 0.250-g sample of calcium metal is heated in a 38.500-g crucible to form calcium oxide. The resulting crucible and product weigh 38.850 g. Refer to Example Exercise 1 and determine the empirical formula of calcium oxide. DATE DATA TABLE A Empirical Formula of Magnesium Oxide mass of crucible and cover + magnesium metal (before heating) mass of crucible and cover mass of magnesium metal mass of crucible and cover + magnesium oxide (after heating ) 0000 mass of...
a sample of titanium with a mass of 6.48g reacts with oxygen to form 10.80 g of the metal oxide. determine the emperical formula of the metal oxide
1. When 2.50 g of copper metal reacts with molecular oxygen, the copper oxide product of the reaction has a mass of 2.81 g. What is the empirical formula of the copper oxide product 2. When 10.8 g of silver was reacted with sulfur. 12.4 grams of product was produced there was only one product). What is the empirical formula of the product? 3. Lysine is a compound composed of carbon, hydrogen, nitrogen and oxygen. When 1.50 g of lysine is burned,...
lithium metal reacts with oxygen gas to form solid lithium oxide express your answer as a chemical equation. identify all of the phases in your answer
A 0.266 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid magnesium oxide. In the laboratory a student weighs the mass of the magnesium oxide collected from this reaction as 0.244 g. What is the percent yield of this reaction?
Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark-brown gas: 2NO(g) + O2(8) - 2NO2(8) In one experiment 1.075 mole of NO is mixed with 0.722 mole of O2. Calculate which of the two reactants is the limiting reagent, and report the number of moles of NO2 produced.
If 0.3785 grams of calcium was completely reated with oxygen gas in the air to form calcium oxide, what mass of calcium would be expected? The reaction is as follows : 2Ca(s) + O2(g)— 2CaO(s)
For this reaction, 26.0 g iron reacts with 6.11 g oxygen gas. iron (s) + oxygen (g) iron(II) oxide (s) What is the maximum mass of iron(II) oxide that can be formed? g What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete?