9.1.00 g of tin (Sn) combines with 0.27 g of oxygen from the air to form...
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...
Anusra ple of tin (1187 e) combines with 10.0 g of sulfur (32.07-i)to form mole compound. What is the empirical formula of this compound? b. SnS2 C. Sn2S
A sample of scandium metal weighing 8.565 g is heated in air and combines with oxygen. The resulting compound weighs 13.137 g. Calculate the following: a. Mass of oxygen reacted? b. Moles of scandium atoms? c. Moles of oxygen atoms? d. The empirical formula of the compound?
A0.500-g sample of tin foil reacted with oxygen to give 0.635 g of product. Calculate the empirical formula of the tin oxide. Refer to Example Exercise 1 Record your numbers to 3 significant figures. Do not use exponential notation or subscripts in your answers. a) The mass of oxygen used in the reaction is b) The number of moles of tin is moles and the number of moles of oxygen is moles. c) Using their ratio of number of moles,...
The element tin often occurs in nature as the oxide, SnO2. In order to produce pure tin metal from this sort of tin ore, the ore is usually heated with coal (carbon). This produces pure molten tin, with the carbon being removed from the reaction system as the gaseous byproduct carbon monoxide. The correct chemical equation for this process is: SnO2(s) + C(s) + heat --> Sn(s) + CO(g) SnO2(s) + C(s) + heat --> Sn(1) + CO(g) SnO2(s) +...
Mass of empty crucible with cover Mass of crucible, cover, and tin Mass of crucible, cover, and sample after reaction and prolonged heating 19.66 g 21.76 g 22.33 g A similar experiment was used to determine the empirical formula of an oxide of tin (Sn). Use the data provided to answer the following question. Calculate the number of moles of tin in the oxide of tin sample. Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and...
5. A 0.565-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide Calculate the empirical formula of the product. 6. A 0.750-g sample of tin foil was heated in air and reacted with oxygen gas to give 0.953 g of tin oxide. Calculate the empirical formula of the product. 7. (optional) A 1.000-g sample of red phosphorus powder was burned in air and reacted with oxygen gas to give 2.291 g of phosphorus oxide. Calculate...
4.72 grams of pure phosphorus are allowed to react with oxygen in air to form an oxide. If the product weights 10.82 grams, find the empirical formula of the compound. Show all steps.
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
Page 5 of 7 0 - 200m + 3. A student follows the Procedure of this experiment to determine the empirical formula for an oxide of tin (Sn), and collects the following data: Mass of crucible 22.368 Mass of Sn Mass of crucible and tin oxide 7.873 31.298 a) Calculate the mass of tin oxide. b) Calculate the mass of O c) Calculate the number of moles of Sn. d) Calculate the number of moles of O e) Write a...