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grades should be 1 1 point If the mass ratio of Mg to Sin a compound...
1 point If the mass ratio of Mg to Sin a compound is 1.8:6.3, how many grams of Sare needed to react with 8.17 g of Mg? Type your answer...
A compound of Cu and S is prepared by heating Cu metal with excess Sin a crucible. The mass of Cu in the compound formed is 2.395 g. And the mass of S in the compound in it is 0.604 g. What is the compound's empirical formula? [Hint: Change grams (element) mole (element) mole ratio (compound)]
Question 4 (1 point) A compound with a molecular mass of 283.88 g/mol is found to contain 43.64 %P and 56.36% O. What is the molecular formula of this compound? OPO4 OP203 P205 OP4010 OPAOG Question 5 (1 point) If (4.544x10^1) g of oxygen react with (4.81x10^1) g of carbon monoxide to form carbon dioxide. What mass of carbon dioxide forms? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Answer
Question (1 point) A compound containing only C. H. and O. was extracted from the bark of the sassafras tree. The combustion of 82.3 mg produced 223 mg of CO2 and 45.8 mg of H20. The molar mass of the compound was 162 g/mol. Determine its empirical and molecular formulas. e See page 299 1st attempt i See Periodic Table Part 1 (0.5 point) Note that formulas of organic compounds should fhrst list the carbon and hydrogen with the rest...
The percentage by mass for element X in a compound is 66%. How many grams of X is needed to 46.4 grams of the compound? ( Do not include the units in your answer)
eRification of a Compound by Mass Relationships 1. A student attempts to identify an unknown compound by the method used in this expeni- ment. She finds that when she heated a sample weighing 0.5015 g the mass went down appreciably, to 0.3432 g. When the product was converted to a chloride, the mass went up, to 0.3726 g. a. Is the sample a carbonate? Give your reasoning. b. What are the two compounds that might be in the unknown? and...
Experiment 7 Empirical Formula Objectives: Determine the expected formula for the ionic oxide expected when Mg reacts with O2 Find the theoretical and actual yields of magnesium oxide Evaluate results using stoichiometry and error analysis Introduction: The goal of this experiment is to determine the Empirical Formula of a Compound. (The Empirical Formula of a Compound is the simplest whole number ratio between the elements of a compound) If one can synthesize a compound from elements, then it is possible...
1) How many moles of Mgo could be produced from 0.15 moles of Mg?! Mg + O2 + Mgo 2) How many moles Fe would be required to produce 2.5 moles of Fe2O,? 4Fe + 302 + 2Fe2O3 3) Determine the mass of CO2 (in grams) that could be produced from 1.55 g of CS2. CS2 + 302 → CO2 + 2502 4) How many grams of NaNO, would be needed to produce 5.0 g of NaNO,? 2NaNO3 + 2NaNO2...
In a chemical reaction, a student react 1.315 grams of elemental Mg solid in the lab (with unlimited amount of oxygen) and produced MgO. 2Mg(s) + O2(g) 2MgO(s) (A) Determine the number of moles of Mg solid used in this reaction? (B) If all the magnesium reacted to form the magnesium oxide, how many moles of magnesium oxide was produced? (C) What mass of magnesium oxide was produced? (D)Name the general type of reaction shown above?
2Mg(s) + O2(9) --> 2Mgº(s) molar mass Mg = 24.30 g/mol molar masso2 = 31.98 g/mol molar mass Mgo = 40.29 g/mol If 12.6 grams of magnesium completely react to form magnesium oxide according to the equation given, how much magnesium oxide is produced?