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

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

Chapter5: The Gaseous State

Section5.2: Empirical Gas Laws

Problem 5.2CC

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Practice Problems 1. A gas has a volume of 350 ml at 30 C. If the volume changes to 400 ml, what is the new temperature? 2. Submarines need to be extremely strong to withstand the extremely high pressure of water pushing down on them. An experimental research submarine with a volume of 1,510 liters has an internal pressure of 1.20atm. If the pressure of the ocean breaks the submarine forming a bubble with a pressure of 253atm pushing on it, how big will that bubble be? 3. A sample of nitrogen inside a rigid, metal container at 20.0ºC is placed inside an oven whose temperature is 50.0 ̊ C. The pressure inside the container at 20.0ºC started at 3.00 atm?
Problem 1.20. Uranium has two common isotopes, with atomic masses of 238 and 235. One way to separate these isotopes is to combine the uranium with fluorine to make uranium hexafluoride gas, UF6, then exploit the difference in the average thermal speeds of molecules containing the different isotopes. Calculate the rms speed of each type of molecule at room temperature, and compare them.
Practice problem: A fixed volume of 5 L is holding 4 moles of gas at a pressure of 3 atm. If the quantity of gas is increased to 5 moles, what will be the new pressure? Practice Problem (You first need to determine which law to use). A 0.4 moles of gas with a volume of 2 L has a T of 413 K and a P of 7 atm. If we decrease the T to 325 K while holding the V constant, what is the new P?
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. If an air bag has a volume of 53.4 L and is to be filled with nitrogen gas at a pressure of 1.07 atm and a temperature of 23.7˚C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas. Answer sig figs
Sodium metal reacts with water according to the following reaction: 2Na(s) + 2H2O(l) --> H2(g) + 2NaOH(aq) How many liters of hydrogen gas (at STP) would be produced from 6.25 g of sodium? Report answer to 3 significant figures.
What is the average kinetic energy (in kJ mol-1) of a hypothetical gas with molecular weight 31.2 g mol-1 at a temperature of 77.1 °C? Do not try to identify the gas. Express answer in 2 significant figures.
The reaction between baking soda and vinegar is;NaHCO3(s) + HC2H3O2(aq)→NaC2H3O2(aq) + H2O(l) + CO2(g) How many grams of baking soda will produce 1.5L of carbon dioxide at 20ᵒC and 655mmHg? (hint; solve PV=nRT for n of CO2 first then use the balanced equation).
Question: - What was WUE = (A/1000) / E What was the average WUE measured at ambient [CO2] in A? and B? (ONLY CORRECT ANSWERS)
In the combustion C6H6O2, what is the value of the slope expected for a) a plote of moles of C6H6O2 (y axis) versus moles of CO2 (x axis), and b) a plot of moles of O2 (y axis) versus moles of H2O (x axis)?
Answer the ff: 1. Write equations for the substitution of hydrogen by bromine in methane and the reaction for the combustion of ethane.2. Give equations for the preparation of methane by two other methods.3. Calculate the volume of air required for the combustion of 2 liters of ethane.
Balanced Equation: Zn + 2HCl → ZnCl2 + H2 Net Ionic Equation: Zn + 2H → Zn2+ + H2 1. If a 0.25 g sample of Zn reacts with excess HCl… How many moles of HCl will react? How many moles of H2(g) should be produced? 2. The experiment takes place under the following conditions: 300 K, Patm = 777 mmHg, PH2O at 300 K = 26.7 mmHg. How many liters of H2 would be generated under these conditions from the reaction of 0.25 g Zn with excess HCl? 3. How would the amount of H2 collected change if the piece of zinc that reacted had a mass of 0.35 g? Explain.
Practice Exercise 1If you fill your car tire to a pressure of 32 psi (pounds persquare inch) on a hot summer day when the temperature is35 °C 195 °F2, what is the pressure (in psi) on a cold winterday when the temperature is -15 °C 15 °F2? Assume no gasleaks out between measurements and the volume of thetire does not change.(a) 38 psi (b) 27 psi (c) -13.7 psi (d) 1.8 psi(e) 13.7 psi

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