if a 0.192g sample of copper metal reacts with elemental sulfer to form 0.240 g of...
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a 0.192g sample of copper metal
reacts with elemental sulfer to form 0.240 g of...
1. A 0.750-g sample of tin metal reacts with 0.201 g of oxygen gas to form tin oxide.
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...
7. A 0.250-g sample of calcium metal is heated in a 38.500-g crucible to form calcium...
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...
1. When 2.50 g of copper metal reacts with molecular oxygen, the copper oxide product of the reaction has a mass of...
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,...
27. A 1.23 g sample of copper metal is reacted completely with chlorine gas to produce...
27. A 1.23 g sample of copper metal is reacted completely with chlorine gas to produce 2.61 g of copper chloride. Determine the empirical formula and empirical formula mass for this compound.
A 0.500-g sample of chromium metal reacted with sulfur powder to give 0.963 g of product. a) The mass of sul...
A 0.500-g sample of chromium metal reacted with sulfur powder to give 0.963 g of product. a) The mass of sulfur that reacted is _____ b) The empirical formula of the chromium sulfide is _____
A 17.59 gram sample of copper is heated in the presence of excess bromine. A metal...
A 17.59 gram sample of copper is heated in the presence of excess bromine. A metal bromide is formed with a mass of 39.71 g. Determine the empirical formula of the metal bromide. Enter the elements in the order Cu, Br empirical formula= A 10.70 gram sample of chromium is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of 22.42 g. Determine the empirical formula of the metal fluoride. Enter the elements in...
6) A sample of a sulfide of a metal M, (formula MxSy), is submitted to analysis...
6) A sample of a sulfide of a metal M, (formula MxSy), is submitted to analysis to identify the metal. The sulfur in the sample is recovered as 120 mL of 0.250 M Na2S solution. The metal in the same sample is recovered as 40.0 mL of 0.500 M solution of the metal ion. a. Find the formula MxSy of this metal sulfide. b. The molar mass of this sulfide is 150 g/mole. Identify the metal The final answer for...
A 26.0 g sample of chromium (Cr) reacts with sulfur (S) to form 50.0 g of chromium sulfide. Determine the formula for th...
A 26.0 g sample of chromium (Cr) reacts with sulfur (S) to form 50.0 g of chromium sulfide. Determine the formula for the chromium sulfide and the charge on the chromium ion. Show work for all steps.
A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of prod...
5. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of prod Calculate the empirical formula of the iron sulfide.6. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.861 g of product Calculate the empirical formula of the iron sulfide.
1. If you began with 0.5296 g of copper mesh and recovered 0.2937 elemental copper, what...
1. If you began with 0.5296 g of copper mesh and recovered 0.2937 elemental copper, what would be the percent recovery of copper metalo 2. Describe the differences in the appearance of the copper mesh vs. the appearance of the elemental copper at the end of the reaction sequen Why should you be careful not to overheat the crude copper metal in the evaporating dish. Which reaction do you think might occur if the sample is heated too strongly? How...
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...
27. A 1.23 g sample of copper metal is reacted completely with chlorine gas to produce 2.61 g of copper chloride. Determine the empirical formula and empirical formula mass for this compound.
A 17.59 gram sample of copper is heated in the presence of excess bromine. A metal bromide is formed with a mass of 39.71 g. Determine the empirical formula of the metal bromide. Enter the elements in the order Cu, Br empirical formula= A 10.70 gram sample of chromium is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of 22.42 g. Determine the empirical formula of the metal fluoride. Enter the elements in...
1. If you began with 0.5296 g of copper mesh and recovered 0.2937 elemental copper, what would be the percent recovery of copper metalo 2. Describe the differences in the appearance of the copper mesh vs. the appearance of the elemental copper at the end of the reaction sequen Why should you be careful not to overheat the crude copper metal in the evaporating dish. Which reaction do you think might occur if the sample is heated too strongly? How...
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