Initial Knowledge Check Question 5 Me Liquid hexane (CH,(CH,) CH,) will react with gaseous oxygen (0,) to produce gaseous carbon dioxide (CO,) and gaseous water (H,O). Suppose 0.86 g of hexane is mixed with 5.93 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant dipits. I Don't Know Submit 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessi enovo III

Initial Knowledge Check Question 5 Me Liquid hexane (CH,(CH,) CH,) will react with gaseous oxygen (0,) to produce gaseous carbon dioxide (CO,) and gaseous water (H,O). Suppose 0.86 g of hexane is mixed with 5.93 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant dipits. I Don't Know Submit 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessi enovo III

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter10: The Mole

Section: Chapter Questions

Problem 213A

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Mass of Copper Oxide: 1.0495g Mass of filter paper: 0.6698g Mass of empty watch glass: 43.2063g Mass of watch glass, filter paper, and solid: 44.7007g Mass of solid copper:_____ Mass of oxygen in the copper oxide:____ A) Determine the empirical formula of the copper oxide (Show all work): B) Determine the mass percent of copper and oxygen in your sample( show all your work):
Use the information given to you below to solve/calcualte the rest of the table. Please show all work on how you reached your answers. Formula of Unknown Hydrate: ? Numbers of Water: 2 Molar mass of Unknown Anhydride: 208.233 g/mol Weight of Hydrate and Evaporating Dish: 62.679 g Weight of Empty Evaporating Dish: 52.655 g Weight of Hydrate: ? Weight of Sample and Evaporating Dish after 1st Heating: 61.199 g Weight of Sample and Evaporating Dish after 2nd Heating: 61.199 g Weight of Sample and Evaporating Dish after 3rd heating: 61.199 g Weight of Anydride and Evaporating Dish: 61.199 g Weight of Water lost: ? Weight of Anhydride: ? Experimental Percent Water: ? Moles of Water: ? Moles of Anhydride: ? Ratio of Moles of Water to Moles of Anhydride: ? Experimental Formula of Hydrate: ? Please show all work on how you came to each answer. Thank you! (place in formula like this-sample- QXRy*ZH2O)
Multiple Choice: If I computed the molar mass of sodium chloride, whereby I can secure the number of particles of sodium chloride (Avogadro's constant) as a compound, what will I do if I want to know how many sodium cations do I have right now? a. compute the molar mass of the sodium to get the Avogadro’s constant number of particles b. none of the choices here are acceptable or correct c. compute the molar mass of chloride ion to get the Avogadro’s constant number of particles d. in computing the molar mass of sodium chloride, to get the Avogadro’s constant number of particles
4.22L of F2 @STP has how many molecules ? round answer to 2 decimal places.
please answer as fast as possible How many oxygen atoms are there in 22.0 g of carbon dioxide? A) 6.02 x1023 ○ B) 1.20 x1024 C) 5.09 x1023 OD) 1.42 x1024 (Please type answer no write by hend)
3. Now let's suppose it's your turn to be the professor. You want to write a question for your students using theoretical data. Suppose you want their "unknown liquid" to be toluene (molar mass = 92.1 g/mol). Using the data in the table below, what should the "mass of flask + unknown condensed liquid" be so that they can correctly identify toluene as their unknown? Mass of flask: 77.485 g Mass of flask + unknown condensed liquid: ????? Temperature of water bath: 100 °C Pressure of gas in our system: 0.997 atm Volume of gas in our system: 255 mL Group of answer choices: A) 78.250 B) 0.765 C) 1.04 g D) 78.525 g
I need help understanding how to complete this question. I have done some of the owrk, hopefully correctly. THe istructions are: Calculate how many moles of CaCl2•2H2O are present in 1.50 g of CaCl2•2H2O and then calculate how many moles of pure CaCl2 are present in the 1.50 g of CaCl2•2H2O. Record the answers in Data Table 1. Use the information and examples provided in the Exploration and the values recorded in Data Table 1 from Step 8 to determine how many moles of Na2CO3 are necessary to reach stoichiometric quantities. From that calculation, determine how many grams of Na2CO3 are necessary to reach stoichiometric quantities. Record both values in Data Table 1. Initial: CaCl2 x 2H20 (g) 1.50 g Initial: CaCl2 x 2H2O (mol) 147.02 g/mol Initial: CaCl2 (mol) 0.0102 mol Initial: NaCO3 (mol) 106 g/mol Initial: NaCO3 (g) Theoretical: CaCO3 1.02 g Mass of filter paper 1.2 g Mass of filter + CaCO3 2.6 g Actual: CaCO3 (g) 1.4 g % yield
Consider the following unbalanced equation: C2H6(g) + O2(g) → CO2(g) + H2O(g) Which amount requires more oxygen gas, 2.35 mol C2H6 or 30.6 g C2H6? What information do we need to determine which amount of C2H6 requires more oxygen gas? Select ALL correct options. Group of answer choices a 2.35 mol C2H6 b molar mass of C2H6 c balanced chemical equation d number of grams present in 1 kilogram e 30.6 g C2H6
1 hi Experts...please help me, i need it until 5:30 pm. Hope you can answer it before the time thank you soo much!. Calculate the number of moles of CaCO3 in 150 g sample of limestone which is 90% pure.
Show ALL work. Remember to follow significant digit rules and show proper format in all answers. NOTE: Record all molar mass values to 2 decimal places. Question: Calculate the mass in grams of 4.25 moles of Ag2S?
Please answer part D PART A) What is the maximum number of moles of P2O5P2O5 that can theoretically be made from 211 gg of P4P4 and excess oxygen? Express your answer to three significant figures and include the appropriate units.=3.40 moL PART B) What is the maximum number of moles of P2O5P2O5 that can theoretically be made from 240 gg of O2O2 and excess phosphorus? Express your answer to three significant figures and include the appropriate units. =3.00moL PART C) In Part A, you found the number of moles of product (3.40 mol P2O5mol P2O5 ) formed from the given amount of phosphorus and excess oxygen. In Part B, you found the number of moles of product (3.00 mol P2O5mol P2O5 ) formed from the given amount of oxygen and excess phosphorus. Now, determine the number of moles of P2O5P2O5 is produced from the given amounts of phosphorus and oxygen. Express your answer to three significant figures and include the appropriate units. =3.00Mol PART D) What is the percent yield if…
Consider the following unbalanced equation: C2H6(g) + O2(g) → CO2(g) + H2O(g) Which amount requires more oxygen gas, 2.35 mol C2H6 or 30.6 g C2H6? What information do we need to determine which amount of C2H6 requires more oxygen gas? Select ALL correct options. Group of answer choices 2.35 mol C2H6 molar mass of C2H6 balanced chemical equation number of grams present in 1 kilogram 30.6 g C2H6