2 words DX Text Predictions: On✓Start VideoescChapter #3 WorksheetA student performs a reaction in which they combine iron (III) oxide with carbon. The reactionproduces carbon dioxide and iron.!1Qa. Write a balanced chemical equation for this reaction.b. How many moles of carbon would be needed to produce 6.35 mol of iron?c. If 18.5 g of carbon dioxide are produced in the reaction, how many moles of iron werealso produced?d. (i) If 3.25 mol of carbon reacts with 115.85 g of iron (III) oxide, how many moles of ironwere produced?A(ii) How many moles of excess reactants were left over?(iii) If 75.9 g of iron were recovered at the end of the experiment, what would be thepercent yield of iron?Accessibility: InvestigateN@2WS#3EParticipants$415X CRD F%5ChatVTShare Screen6RecordYB&7Live Transcript* 00Reactions89G H J K69□Apps WhiteboardsFocusN M00O)0VL0P

a.) Balanced reaction can be written as per given Reactants and products. b.) To calculate the…

A student performs a reaction in which they combine iron (III) oxide with carbon. The reaction produces carbon dioxide and iron. a. Write a balanced chemical equation for this reaction. b. How many moles of carbon would be needed to produce 6.35 mol of iron? c. If 18.5 g of carbon dioxide are produced in the reaction, how many moles of iron were also produced?

A student performs a reaction in which they combine iron (III) oxide with carbon. The reaction produces carbon dioxide and iron. a. Write a balanced chemical equation for this reaction. b. How many moles of carbon would be needed to produce 6.35 mol of iron? c. If 18.5 g of carbon dioxide are produced in the reaction, how many moles of iron were also produced?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 70QAP: The first step in the manufacture of nitric acid by the Ostwald process is the reaction of ammonia...

See similar textbooks

Similar questions

DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
Chlorine and fluorine react to form gaseous chlorine trifluoride. Initially, 1.75 mol of chlorine and 3.68 mol of fluorine are combined. (Assume 100% yield for the reaction.) (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of chlorine trifluoride in moles? (d) How many moles of excess reactant remain after reaction is complete.
Sand is mainly silicon dioxide. When sand is heated with an excess of coke (carbon), pure silicon and carbon monoxide are produced. (a) Write a balanced equation for the reaction. (b) How many moles of silicon dioxide are required to form 20.00 g of silicon? (c) How many grams of carbon monoxide are formed when 98.76 g of silicon are produced?
Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. C2N2(g)+7F2(g)2CF4(g)+2NF3(g)(a) How many moles of fluorine react with 1.37 mol of cyanogen? (b) How many moles of CF4 are obtained from 13.75 mol of fluorine? (c) How many moles of cyanogen are required to produce 0.8974 mol of NF3? (d) How many moles of fluorine will yield 4.981 mol of nitrogen trifluoride?
Hydrazine N2H4, emits a large quantity of energy when it reacts with oxygen, which has led to hydrazine’s use as a fuel for rockets: :math>N2H4(l)+O2(g)N2(g)+2H2O(g) w many moles of each of the gaseous products are produced when 20.0 g of pure hydrazine ¡s ignited in the presence of 20.0 g of pure oxygen? How many grams of each product are produced?
When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. :math>C(s)+O2(g)CO2(g) wever, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. :math>2C(s)+O2(g)CO(g) at mass of each product is expected when a 5.00-g sample of pure carbon is burned under each of these conditions?
itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is C63H88CoN14O14P . A lack of this vita min in the diet can lead to anemia. Cyanocohalamin is the form of the vitamin found in vitamin supplements. l type='a'> What is the molar mass of cyanocobalamin to two decimal places? How many moles of cyanocohalamin molecules are present in 250 mg of cyanocobalamin? What is the mass of 0.60 mole of cyanocobalamin? How many atoms of hydrogen are in 1 .0 mole of cyanocobalamin? What is the mass of 1.0107 molecules of cyanocobalamin? What is the mass (in grams) of one molecule of cyanocobalamin?
The first step in the manufacture of nitric acid by the Ostwald process is the reaction of ammonia gas with oxygen, producing nitrogen oxide and steam. The reaction mixture contains 7.60 g of ammonia and 10.00 g of oxygen. After the reaction is complete, 6.22 g of nitrogen oxide are obtained. (a) Write a balanced equation for the reaction. (b) How many grams of nitrogen oxide can be theoretically obtained? (c) How many grams of excess reactant are theoretically unused? (d) What is the percent yield of the reaction?
Copper(I) iodide (CuI) is often added to table salt as a dietary source of iodine. How many moles of CuI Are contained in 1.00 lb (454 g) of table salt containing 0.0100% CuI by mass?
An air bag is deployed by utilizing the following re tion the nitrogen gas produced inflates the air bag): :math>2NaN3(s)2Na(s)+3N2(g) 10.5 g of NaN1 is decomposed, what theoretical mass of sodium should be produced? If only 2.84 g of sodium is actually collected, what is the percent yield?
When solid phosphorus (P4) reacts with oxygen gas, diphosphorus pentoxide is formed. Initially 2.87 mol of phosphorus and 3.86 mol of oxygen are combined. (Assume 100% yield.) (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) How many moles of excess reactant remain after the reaction is complete?
The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen. (a) What is the limiting reactant when 0.200 mol of P4 and 0.200 mol of 02 react according to P4+5O2P4O10 (b) Calculate the percent yield if 10.0 g of P4O10 is isolated from the reaction.