For the equation P4 (s) + 502 (g) →→ P4O10 (s), if 3 mol of phosphorus react with 10 mol of oxygen gas, the theoretical yield of tetraphosphorus decaoxide will be а. 1 mol. b. 2 mol. с. 3 mol. d. 10 mol. O A Ов O D

Ammonia gas can be prepared by the reaction CaO(s) + 2NH4Cl(s) → 2 NH3(g) + H₂O(g) + CaCl₂ (s) In an experiment, 33.0 g of ammonia gas, NH3, is produced when it was predicted that 43.2 g NH3 would form. What is the theoretical yield of NH3 ? theoretical yield: What is the actual yield of NH3 ? actual yield: What is the percent yield of NH3 ? percent yield: 6.0 g 0.0 g %

A MOving tổ another question WIII Save Question 3 Cobalt reacts with excess oxygen gas to form colbalt(III) oxide. Choose the correct representation of this reaction. A. Co + 02 → Co203 B. 4 Co + 3 02 → 2 Co2O3 C. 2 Co + O2 → 2 CoO D.3 Co + O2 → Co3O2 A A Moving to another question will save this response. 0,432 11 éty P MacBook Pro $ * 3 4. 5 7 8 CO

Hydrocarbons such as propane burn in oxygen gas to produce heat. The balanced equation below shows the complete combustion of propane in oxygen. C3H₂(g) +50₂(g) → 3C0₂(g) + 4H₂O(g) How many moles of O₂ would be needed to cause the complete combustion of 3.00 g C3H8? moles

How many molecules of carbon monoxide (CO) are needed to react with excess iron (III) oxide (Fe₂O 2 3) to produce 11.6 g of iron (Fe)? Fe₂O₂ +3CO→2Fe + 3CO A 11.6 molecules CO FR [] U D 6.02 x 10 molecules of CO 1.88 x 10² molecules of CO 2.0 molecules CO

a. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.355 mol of the first reactant. Cl₂(g) + KI(aq) → I₂ (s) + KCl(aq) mol KI b. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.400 mol of the first reactant. Co(s) + P4 (8)→ C03 P2 (8) mol P4 c. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.215 mol of the first reactant. Zn(s) + HNO3(aq) → Zn(NO3)2 (aq) + H₂ (9) mol HNO3 d. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.370 mol of the first reactant. C5 H12 (1) + O2(g) → CO2 (g) + H₂O(g) mol O2

In each chemical reaction below, an atom or group of atoms is moving. It is bonded to something different in the reactants than it is in the products. A chemical reaction always involves a move like this. 18. A. B. C. D. 19. PAAUA ARCA D. 20. A. B. C. 9.1 0Z (258g) D. 4 H2 + CO2 → CH4 + 2 H₂O mie Which atoms is the C bonded to in the reactants? (C) Which atoms is the C bonded to in the products? en (H) Which atom is each O bonded to in the reactants? (0) Which atoms is each O bonded to in the products? (C) HCl + NaOH → NaCl + HOH Which atom is the Cl bonded to in the reactants? Which atom is the Cl bonded to in the products? Which atom is the OH group bonded to in the reactants? Which atom is the OH group bonded to in the products? will pieces to leave all CH4 + 2 O2 CO₂ + 2 H₂Oith the labi, please Which atom is the C bonded to in the reactants? Which atom is the C bonded to in the products? Which atom is the O bonded to in the reactants? Which atom is the O bonded to in the products?…

a. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.255 mol of the first reactant. AgNO3(aq) + LiOH(aq) → AgOH(s) + LiNO3(aq) g AgOH g LiNO3 b. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.155 mol of the first reactant. Al2(SO4)3(aq) + 3CaCl2 (aq) → 2AlCl3 (aq) + 3CaSO4 (8) g AICI, g CaSO4 c. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.215 mol of the first reactant. CaCO3 (8) + 2HCl(aq) → CaCl₂ (aq) + CO₂(g) + H₂O(1) g CaCl₂ g CO2 g H₂O ubmit Answer Retry Entire Group 9 more group attempts remaining Show Hint Previous Next

12. Iron metal can be obtained from iron(III) oxide by reaction with carbon monoxide at elevated temperature according to the following equation. Fe203 + 3CO → 2Fe + 3CO2 a. How many moles of iron can be obtained from 1 mole of iron(III) oxide? b. How many grams of Fe2O3 are necessary to make 50 g of iron by this reaction?

For the reaction 2KClO3(s)→2KCl(s)+3O2(g) calculate how many grams of oxygen form when each quantity of reactant completely reacts. a) 2.12 gKClO3gKClO3   b) 0.354 gKClO3 c) 82.7 kgKClO3 d) 29.9 mgKClO3