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II Review | Constants I Periodic Table Butane, C4 H10, reacts with oxygen, O2 , to form water, H2 O, and carbon dioxide, CO2 , as shown in the following chemical equation: Now that you know the molar masses of the relevant compounds, you are ready to start solving stoichiometry problems. In general, the typical strategy is 1. Convert from grams of compound X to moles of compound X using the molar mass of compound X. 2. Convert from moles of compound X to moles of compound Y using the coefficients in the balanced chemical equation. 3. Convert from moles of compound Y to grams of compound Y using the molar mass of compound Y. 2C4H10 (g) + 1302(g)→10H2O(g) +8CO2(g) The coefficients in this equation represent mole ratios. Notice that the coefficient for water (10) is five times that of butane (2). Thus, the number of moles of water produced is five times the number of moles of butane that react. Also, notice that the coefficient for butane (2) is one- fourth the coefficient of carbon dioxide (8). Thus, the number of moles of butane that react is one-fourth Part B the number of moles of carbon dioxide that you produce. But be careful! If you are given the mass of a compound, you must first convert to moles before applying these ratios. Calculate the mass of water produced when 6.65 g of butane reacts with excess oxygen. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HẢ Value Units Submit Part C Calculate the mass of butane needed to produce 71.4 g of carbon dioxide. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ? Value Units Submit

II Review | Constants I Periodic Table Butane, C4 H10, reacts with oxygen, O2 , to form water, H2 O, and carbon dioxide, CO2 , as shown in the following chemical equation: Now that you know the molar masses of the relevant compounds, you are ready to start solving stoichiometry problems. In general, the typical strategy is 1. Convert from grams of compound X to moles of compound X using the molar mass of compound X. 2. Convert from moles of compound X to moles of compound Y using the coefficients in the balanced chemical equation. 3. Convert from moles of compound Y to grams of compound Y using the molar mass of compound Y. 2C4H10 (g) + 1302(g)→10H2O(g) +8CO2(g) The coefficients in this equation represent mole ratios. Notice that the coefficient for water (10) is five times that of butane (2). Thus, the number of moles of water produced is five times the number of moles of butane that react. Also, notice that the coefficient for butane (2) is one- fourth the coefficient of carbon dioxide (8). Thus, the number of moles of butane that react is one-fourth Part B the number of moles of carbon dioxide that you produce. But be careful! If you are given the mass of a compound, you must first convert to moles before applying these ratios. Calculate the mass of water produced when 6.65 g of butane reacts with excess oxygen. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HẢ Value Units Submit Part C Calculate the mass of butane needed to produce 71.4 g of carbon dioxide. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ? Value Units Submit

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter3: Calculations With Chemical Formulas And Equaitons
Section: Chapter Questions
Problem 3.141QP: A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume...
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I Review I Constants I Periodic Table Butane, C4H10, reacts with oxygen, O2 , to form water, H20, and carbon dioxide, CO2 , as shown in the following chemical equation: Now that you know the molar masses of the relevant compounds, you are ready to start solving stoichiometry problems. In general, the typical strategy is 2C,H10 (g) + 1302(g)→10H2O(g) +8CO2 (g) The coefficients in this equation represent mole ratios. Notice that the coefficient for water (10) is five times that of butane (2). Thus, the number of moles of water produced is five times the number of moles of butane that react. 1. Convert from grams of compound X to moles of compound X using the molar mass of compound X. 2. Convert from moles of compound X to moles of compound Y using the coefficients in the balanced chemical equation. 3. Convert from moles of compound Y to grams of compound Y using the molar mass of compound Y. Also, notice that the coefficient for butane (2) is one- fourth the coefficient of carbon dioxide (8). Thus, the number of moles of butane that react is one-fourth Part B the number of moles of carbon dioxide that you Calculate the mass of water produced when 6.65 excess oxygen. of butane reacts with produce. But be careful! If you are given the mass of a compound, you must first convert to moles before applying these ratios. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units Submit Part C Calculate the mass of butane needed to produce 71.4 g of carbon dioxide. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HẢ ? Value Units Submit
Transcribed Image Text:I Review I Constants I Periodic Table Butane, C4H10, reacts with oxygen, O2 , to form water, H20, and carbon dioxide, CO2 , as shown in the following chemical equation: Now that you know the molar masses of the relevant compounds, you are ready to start solving stoichiometry problems. In general, the typical strategy is 2C,H10 (g) + 1302(g)→10H2O(g) +8CO2 (g) The coefficients in this equation represent mole ratios. Notice that the coefficient for water (10) is five times that of butane (2). Thus, the number of moles of water produced is five times the number of moles of butane that react. 1. Convert from grams of compound X to moles of compound X using the molar mass of compound X. 2. Convert from moles of compound X to moles of compound Y using the coefficients in the balanced chemical equation. 3. Convert from moles of compound Y to grams of compound Y using the molar mass of compound Y. Also, notice that the coefficient for butane (2) is one- fourth the coefficient of carbon dioxide (8). Thus, the number of moles of butane that react is one-fourth Part B the number of moles of carbon dioxide that you Calculate the mass of water produced when 6.65 excess oxygen. of butane reacts with produce. But be careful! If you are given the mass of a compound, you must first convert to moles before applying these ratios. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units Submit Part C Calculate the mass of butane needed to produce 71.4 g of carbon dioxide. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HẢ ? Value Units Submit
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