rences) A few hydrogen and oxygen molecules are introduced into a container in the quantities depicted in the following drawing. The gases are then ignited by a spark, causing them to react and form H2O. H2 a. Write a balanced chemical equation for the reaction. (Use the lowest possible coefficients. Omit states of matter.) b. What is the limiting reactant? O2 H2 There is no limiting reactant. c. What is the maximum number of water molecules that can be formed in the chemical reaction? water molecules

rences) A few hydrogen and oxygen molecules are introduced into a container in the quantities depicted in the following drawing. The gases are then ignited by a spark, causing them to react and form H2O. H2 a. Write a balanced chemical equation for the reaction. (Use the lowest possible coefficients. Omit states of matter.) b. What is the limiting reactant? O2 H2 There is no limiting reactant. c. What is the maximum number of water molecules that can be formed in the chemical reaction? water molecules

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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29. Consider the following balanced equation: 2N₂O5 ‒‒‒‒‒‒‒> 4NO₂ How many moles of N₂0s are required to produce 62.7 g of NO₂ ? b. 2.73 mol e. 0.681 mol a. 73.6 mol d. 0.00631 mol + O₂ C. 1.36 mol
Mass of crucible and cover 12.73g 2. Mass of crucible, cover, and sample 24.11g 3. Mass of original sample 24.11- 12.73g= 11.97g 4. Mass of crucible, cover, and sample after 1st heating 20.01g 6. Mass of crucible, cover, and sample after 2nd heating (assume that this step was done) 19.98 g 7. Total mass lost by sample during heating what is the percentage of water in the sample? and what is the total mass lost by the sample?
Consider the generic chemical equation: 2 A + 4 B --------> 3 C 1. If 10.0 moles of each reactant were used to complete that reaction, which of the following is true. a. A is the limiting reactant and 15.0 moles of C will be produced. b. A is the limiting reactant and 20.0 moles of C will be produced. c. B is the limiting reactant and 7.50 moles of C will be produced. d. B is the limiting reactant and 22.5 moles of C will be produced. 2. What is the percent yield of this reaction if 6.40 moles of C were actually produced?
Iron oxide reacts with carbon to produce elemental iron and carbon monoxide according the the equation shown below. Consider the reaction of 51.4 grams of Fe2O3 with 24.98 grams of C to produce 19.20 grams of Fe. Fe2O3(s)+3c(s)-------2Fe(s)+3CO(g) a. actual yield b. theoretical yield c. percent yield
61. Consider the reaction between calcium oxide and carbon dioxide: CaO(s) + CO2(g) →→ CaCO3(s) A chemist allows 14.4 g of CaO and 13.8 g of CO₂ to react. When the reaction is finished, the chemist collects 19.4 g of CaCO3. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.
Consider the following chemical reaction: Fe (s) + O2(g) ---------> Fe2O3(s) 2.00 moles of iron is reacted with oxygen gas. Calculate moles of the product. A.) 4.00 moles B.) 0.500 moles C.) 2.00 moles D.) 1.00 moles
10.Which of the following statements is TRUE for the chemical equation given below in which nitrogen gas reacts with hydrogen gas to form ammonia gas assuming the reaction goes to completion? N2 + H2 NH3 A. The reaction of three moles of hydrogen gas will produce 34 g of ammonia. B. One mole of N2 will produce one moles of NH3. C. One mole of nitrogen produces 6.02 x 1023 molecules of ammonia. D. The reaction of one mole of H2 will produce 1/2 moles of NH3.
2. Octane (a common organic solvent, and a major component of gasoline, mol formula: C8H18) burns in the presence of oxygen. The combustion produces carbon dioxide, water, and heat. If we burn 325.2 g of octane, determine: a. The balanced chemical equation for the combustion reaction (you can omit heat) b. The mass of oxygen consumed in the reaction
Sodium and chlorine react to form sodium chloride: What is the theoretical yield of sodium chloride for the reaction of 32.0 g Na with 107.2 g Cl2? A. 1.40 x 104 g NaCl B. 35.4 g NaCl C. 122 g NaCl D. 81.2 g NaCl
3. Consider the following balanced reaction: 2 Fe + 3 Cl₂ → 2 FeCl3 Given 60.0 g of Fe and excess Cl₂ (as much as we need), calculate: a. The theoretical yield of FeCl3, in grams. b. The theoretical amount of Cl₂ consumed, in grams.
carbon 12.01 hydrogen 1.01 oxygen 16.00 A chemist will use a sample of 30 g of ethanol (CH3CH2OH) in an experiment. In one to two sentences, make and justify a claim about the number of moles of ethanol the chemist will use.
5. Using the chemical equation: COg) + 2 H2(g) → CH3OH) a. Starting with 12.5 g H2 and 74.1 g CO, which is limiting reactant? b. What mass of methanol can be obtained (in theory)? c. What mass of the excess reactant is left over?