Question 51 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | 16 | 17 | 18AlomioH Symbol[Hition]1000g weight2 LIВоfuthium Baryum39412MgSodum Tilgan122.190.4119113 Na4 KC SolidHg LiquidH GasRf UnknownMetalsLanthanolds(Lanthanides)24CrActinolds(Actinides)20 2122Ca Sc TiMnCalcm Scandum Thanium Vanadun Oromun Marger4007449 47667 [20902150 140Nonmetals26Fo293027 128Co Ni Cu ZnCoba Nickel Copper neMUSEL en Bola S140Boron194113AlA14SIPretpreNCarbon Navod12,011 140015Pcon Postina Sutr31 $32 133Ga Go AsCan eru Arsen12Jam 125010NoCygen Fome NeonISO 900 $200418Ar16HoFekeMOR34Se17CIChoree3536Br KrPSKryskonGiven the reaction:C8H16+02->__CO₂ + H₂OHow many moles of C8H16 are used when 15.55 liters of C8H16 gas are used, measured atSTP, in an excess of oxygen?Give two decimal places in your answer and no units.

To solve this problem we have to balance the given equation . And calculate the mole of C8H16 used…

Given the reaction: C8H16+ O2--> __CO₂ + H₂O How many moles of C8H16 are used when 15.55 liters of C8H16 gas are used, measured at STP, in an excess of oxygen? Give two decimal places in your answer and no units.

Given the reaction: C8H16+ O2--> __CO₂ + H₂O How many moles of C8H16 are used when 15.55 liters of C8H16 gas are used, measured at STP, in an excess of oxygen? Give two decimal places in your answer and no units.

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...

See similar textbooks

Similar questions

Calculate the density of freon -12 (CF2Cl2) at 26.9 oC and 1.143 atm. density = ___ g/L
Q1: 1. Convert 562 mmHg to KPa? 2. State the following gas law in words and also in the form of an equation: Avogadro's law? 3.Solid has ........ Density. 4. At STP, 0.280L of a gas weighs 0.400 g. Calculate the molar mass of the gas.. Q2: A 36.4-L volume of methane gas is heated from 25°C to 88°C at constant pressure. What is the final volume of the gas??
7 Use significant figures in your answers. 1 NO(g) + 1 H2(g)--> 1 N₂(g) + 1 H₂O(g) 22.15 grams of NO reacts with 2.78 grams of H₂, how many liters of N₂ will be generated at 29.2°C and an atmospheric pressure of 2.01 atm. HINT: Determine the limiting reagent first.
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al(s) + 6 HC1(aq) 2 AICI, (aq) + 3 H, (g) What volume of H, (g) is produced when 7.10 g Al(s) reacts at STP? volume of H, (g):
collected Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. gas chemical reaction water Suppose the 0, gas evolved by a certain chemical reaction taking place at 50.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 58.2 mL. Sketch of a gas-collection apparatus alo Calculate the mass of O, that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. ? Explanation Check © 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility
1.383 moles of lithium react according to the equation below: 2Li(s) + 2H;0() → 2LİOH(ag) + H;(g) [R = 0.0821 atm.L/mol.K) Select the correct operation for calculating the number of moles of H2: The number of moles of Hz is - • unit = Select the correct operation for calculating the volume of 0.6913 mol of H2 at 1.943 atm and 305 K: The volume of H2 gas produced is = * unit - cm3 L Kg g/ml. mL
Type here to search 12 ? 1 o A chemical reaction is shown: 2NO(g) + O₂(g) → 2NO₂(g). How many liters of pure oxygen gas, measured at STP, are required for the complete reaction with 8.82 L of NO(g), also measured at STP? O 4.41L O 11.2L O 17.6L O 882L 0 2241 eTextbook and Media Save for Later Attempts: 0 of 2 used Submit Answer $ A @ (77) A H N @ 2 * W S f3 # X alt 3 2 E D $ 4 C O R F % 5 V T G 40 6 B Y 4 & 7 hp 44 * U H J N 8 19 M a 144 fio ► 11 9 KL < O ➤➤ P 니 . - S alt 112 { ? - + [ " 1 = ( insert. ← ctrl ] U pause 4 4:59 4/30/ prt sc backspace <
The combustion of fuel in your car engine requires oxygen gas, which is supplied as air (21% oxygen molecules) into the engine. Consider a car that is using 100% ethanol, C2H5OH, as fuel. If your engine intakes 2.71 L of air per minute at 1.00 atm and 25ºC, what is the maximum volume of ethanol (0.789 g/mL) that can be burned per minute? Hint: You can ignore the "per minute" information because both the ethanol and air are being quantified per minute. Enter the answer to three significant figures in units of mL.
For the equation below, if you started with 32.6 L of B₂H4 gas at 2.1 atm and 25°C, and your reaction went in 35% yield, how many molecules of product did you isolate? B₂H4 + 2 HF --> 2 BH₂F Please note: If you examine the equation carefully, you will see that it is not balanced correctly (and in fact cannot be balanced). Nevertheless, do NOT correct the coefficients or the chemical substances. Use the equation as it has been given to you. a. 5.9 X 1023 molecules b. 1.2 X 1024 molecules c. 9.6 X 1024 molecules d. 3.8 X 1025 molecules
Automobile airbags inflate following serious impacts, which trigger the chemical reaction:2 NaN3(s) --------> 2 Na(s) + 3 N2(g)If an automobile airbag has a volume of 11.8 L, what mass of NaN3 (in g) is required to fully inflate the airbag upon impact? Assume STP conditions.
19 Linolenic acid (C18H30O2) can be hydrogenated to stearic acid by reacting it with hydrogen gas according to the equation: C18H30O2 (s)+ 3H2 (g)-> C18H36O2 (s) What volume of hydrogen gas (in L), measured at STP, is required to react with 15.3 g of linolenic acid in this reaction?
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. collected gas chemical water reaction Suppose the C0, gas evolved by a certain chemical reaction taking place at 45.0 °C is collected over water, using 圖 an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 32.9 mL. Sketch of a gas-collection apparatus Calculate the mass of CO, that is in the collection tube, Round your answer to 2 significant digits, You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. Help Explanation Check étv 30 DII 110 F7 F3 & 24 % 09 %23 7 5 2 3