Problem 11 K 11 of Review I Constants I Periodic Butane, C4H10, reacts with oxygen, O2, to form water, H2 O, and carbon dioxide, CO2, as shown in the following chemical equation: Submit Previous Answers 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. Correct Part C 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 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 butane needed to produce 61.4 g of carbon dioxide. Express your answer to three significant figures and include the appropriate units. View Available Hint(s) ? HA Units Value Submit P Pearson Privacy Policy | Permissions | Contact Us Copyright 2019 Pearson Education Inc. All rights reserved.| Terms of Use t

Problem 11 K 11 of Review I Constants I Periodic Butane, C4H10, reacts with oxygen, O2, to form water, H2 O, and carbon dioxide, CO2, as shown in the following chemical equation: Submit Previous Answers 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. Correct Part C 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 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 butane needed to produce 61.4 g of carbon dioxide. Express your answer to three significant figures and include the appropriate units. View Available Hint(s) ? HA Units Value Submit P Pearson Privacy Policy | Permissions | Contact Us Copyright 2019 Pearson Education Inc. All rights reserved.| Terms of Use t

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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Apply the significant figure rules to the final answer. The rules are attached. The final answer will not be 5.73.
the statement or answers I) What is the coefficient of CO2 gas after balancing the following equation? KHCO3(6)K2CO3(6) + LH20(8) + _CO2(8) A) 1 B) 2 C) 3 D) 4 E) none of the above - k-2 H- 2 2 C0-3 2) How many moles of H2 can be made from complete reaction of 3.0 moles of Al? Given: 2 Al + 6 HCI-2 AIC13 + 3 H2 A) 9.0 moles B) 3 moles C) 3.0 moles D) 4.5 moles E) none of the above 3) Hydrochloric acid reacts with barium hydroxide according to the equation: 2 HCI (aq) + Ba(OH)2 (aq) - BaCl2 (aq) + 2 H20 (1) AH = -118 kJ Calculate the heat (in kJ) associated with the complete reaction of 54.7 grams of HCI (aq). AY -236 B) F177 C) -88.5 D) -177 E) none of the above 4) Which of the following symbolizes a precipitate in a chemical reaction? A) (s) B) () C) 8) D) (aq) E) none of the above 5) Which of the following statements best describes the following reaction? BaCO3(s), BaO(s) + CO2(8) A) Heating barium carbonate produces barium oxide and carbon dioxide gas. B) Heating barium carbonate…
SKILL #3 CONVERSIONS WITH MOLE RATIO + 50, 2(g) → 3 CO. 2(g) + 4 H,0, (), How many moles of H,0 are produced if 13.8 moles of CO, were produced?
i need answer for all options are in one of the pictures
Limiting Reacting Practice How many grams of silver, Ag, can be formed from 50.8 grams of calcium, Ca, and 1.55 L of 1.51 M silver nitrate solution, AgNO3? (Atomic mass of calcium = 40.08 g/mol, Atomic mass of silver = 107.9 g/mol)
A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr. C6H6 + Br2 --> C6H5Br + HBr What is the theoretical yield of bromobenzene in this reaction when 26.4 g of benzene reacts with 73.6 g of bromine? Answer: ___________ grams Which chemical is the limiting reactant? If the actual yield of bromobenzene was 33.2 g, what was the percent yield? Answer: ____________ %
PRACTICE EXERCISE Balance these equations by providing the missing coefficients: (a) – Fe(s) + – 0;(g) –→ – Fe,O3(s) (b) – C¿H¼(g) + _0;(g) → – CO2(g) + – H;O(g) (c) – Al(s) + _HCl(aq) → – AlCl3(aq) + _H;(g) - -
Question 2 of 16 How many moles of H2SO. are required to completely react with 7.20 mol of AlI according to the balanced chemical reaction: Al(s) + H2SO (aq)A:(SO4)s(aq) + 3 H2(g) STARTING AMOUNT ANSWER RESET ADD FACTOR *( ) 1 26.98 98.08 21.6 342.14 3 7.20 10.8 2.02 6.022 x 1023 2.40 3.60 O Type here to search
The balanced reaction of calcium carbonate and hydrochloric acid is as follows: CACO3 (s) + 2 HC1(aq) → CaCl2 (aq) + H2O (1)+ CO2 (g) Reaction equation of calcium carbonate and hydrochloric acid producing calcium chloride, water and carbon dioxide as products Record your moles and percent error calculations for calcium carbonate Trial 1 Trial 2 Trial 3 Value of CaCO3 reported 500 on the bottle (mg) Mass of antacid tablet used (g) 1.22 1.21 1.22 Moles of HCl from part I. .015000 .015000 .015000 Unrounded Moles of NaOH from part II. .0038610 .0039000 .0037080 Unrounded Moles of HCl neutralized by NaOH .011139 Unrounded Moles of HCl neutralized by NaOH Rounded Moles of HCl neutralized by CaCОз Unrounded Moles of HCl neutralized by CaCOз Rounded Moles of CaCO3 Unrounded Moles of CaCO3 Rounded Mass of CaCO3 in tablet (mg) Unrounded Mass of CaCO3 in tablet (mg) Rounded Percent error (%, use rounded values) Unrounded Percent error (%) Rounded Percent effectiveness of tablet (%) Unrounded…
Following stoichiometry problem step by step on a sheet of paper or white board explaining each step in great detail. Where did you get each number? What is the final answer? Pay attention to sig figs also. Upload your recording. C4H8(g) + 6 O2(g) ⟶⟶4 CO2(g) + 4 H2O(g) Using the reaction above, show and explain on video how many liters of carbon dioxide can be created if I start with 0.2495 grams of C4H8 gas at STP?