Initial Mass of Lighter before experiment22.24gFinal Mass of Lighter after experiment22.01gMass of butane transferred to thegraduated cylinderVolume of butane in graduated cylinder0.23 g100.0 mLAtmospheric Pressure755 mm HgTemperature of water and gas22°CKVapor Pressure of water at 22°C19.8 mm HgPressure of Dry gas0.23 atm Using the formula for butane, C4H10, the ACTUAL molar mass of butane.

We have to calculate molar mass of butane using its formula C4H10

Answered: sing the formula for butane, C4H10, the…

Science

Chemistry

sing the formula for butane, C4H10, the ACTUAL molar mass of butane.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter1: Chemistry: An Introduction

Section1.3: Learning Chemistry

Problem 3RQ

See similar textbooks

Related questions

Q: A beaker contains 5.75 x 1024 molecules of ethanol. How many moles of ethanol are there in a beaker?

Q: Calculate the number of moles of butane, C4H10, in 151 g of butane.

A: Step : 1 Calculate the number of moles of butane, C4H10, in 151 g of butane.

Q: Calculate the mass in grams of 1.23×10241.23×1024 molecules of methanol. The chemical formula for…

A: Given that, the molecules of methanol= 1.23 × 1024 Now, as per Avogadro’s law: 1 mol of methanol…

Q: Caffeine, a stimulant of the central nervous system, has the molecular formula C8H₁0N4O2. The molar…

A: Mass of 1 mole = molar mass 1 mole AB contain 1 mole A and 1 mole B

Q: Calculate the mass in grams of 1.90×10241.90×1024 molecules of Butane, C4H10.

A: Given: Molecules of butane =1.90×10241.90×1024 molecules Standard data: The molar mass of butane…

Q: The chemical formula for chlorophyll is C₅₅H₇₂MgN₄O₅. Given the molar mass of the compound is 893.49…

A: The chemical formula for chlorophyll is C₅₅H₇₂MgN₄O₅. Molar mass of chlorophyll is 893.49 g/mol1 mol…

Q: The mole is defined as the number of atoms in exactly 12 gg of carbon-12. The mole equals…

A: Avogadro number is the unit used for 1 mole of chemical substance. It is applied to convert the…

Q: Determine the number of molecules of ethanol( C 2 H 5 OH) in 47.0 g.

A: In the International System of Units, the mole (symbol: mol) is the unit of measurement for the…

Q: Calculate the mass in grams of 3.07×10243.07×1024 molecules of propane. The chemical formula for…

A: Given that : The number of molecules of propane = 3.07×1024 The chemical formula for propane is…

Q: What is the molar mass of zinc sulfate heptahydrate, ZnSO4·7H2O?

A: We have to calculate the molar mass of zinc sulfate heptahydrate ZnSO4·7H2O

Q: Calculate the mass in grams of 4.46×1024 molecules of propylamine. The chemical formula for…

A: Avogadro constant = 6.022 × 10²³ /mol The moles of propylamine can be calculated asNo. of moles of…

Q: The empirical formula of codeine is C18H21NO3. If the molar mass of codeine is 299 g/mol, what is…

A: In this question empirical formula of codeine is given and we want to determine the Molecular…

Q: Calculate the mass in grams 5.40•1024 molecules of propane. The chemical formula for propane is…

A: The chemical formula of propane is C3H8. Chemical formula of a compound indicates 1 mole of its…

Q: The chemical formula for chlorophyll is C₅₅H₇₂MgN₄O₅. Given the molar mass of the compound is 893.49…

A: Given, mass of C₅₅H₇₂MgN₄O₅. = 1.501 g Molar mass of C₅₅H₇₂MgN₄O₅. = 893.49 g/mol Number of moles =…

Q: How many H atoms are in 75.7 g of acetaldehyde, C2H4O?

Q: What is the mass of 5.83 ×1017 molecules of liquid propane, C3H8?

A: Given, Number of molecules of C3H8 = 5.83 x 1017 Molar mass of C3H8 = 44.1 g/mol First, we find the…

Q: = carbon atoms or

Q: What is the mass of 29.4 mol of benzene (C6H6)?

A: Mole is a unit of measurement to represent the amount of substance. It can be expressed as,…

Q: he molar mass of the hydrate, Co(NO,), · 6H,0.

Q: How many carbon atoms are there in 180 g of propanol (C3H8O).

A: Given mass of propanol

Q: Vitamin B12, cyanocobalamin, is essential for human nutrition. Its molecular formula is…

A: Cyanocobalamin is vitamin B12 with molar mass of 1355.38 g/mol

Q: What is the mass, in grams, of 9.43×1024 molecules of methanol (CH3OH)?

A: Calculate for number of moles of CH3OH: 1 mole of any substance contains 6.022×1023 units (namely…

Q: What is the total mass of oxygen contained in 5.2 g of benzoic acid (C6H5COOH)?

A: This is mole concept reactions

Q: Calculate the mass in grams of 4.66×10244.66×1024 molecules of propane. The chemical formula for…

A: The question is based on mole concept. we have been given molecules of propane. we have to calculate…

Q: A molecule has an empirical formula of CH 2O and a molar mass of 179.9 g/mol. What is the molecular…

A: The empirical formula describes the smallest whole number ratio of atoms present in a compound.…

Q: How many chloride atoms are in 32.3 g of CaCl2?

A: Since you have posted multiple questions, we are entitled to answer the first only. Please repost…

Q: If the empirical formula of a compound is CH2 and its molar mass is 42g/mol, what is its molecular…

A: We know that relation between Molecular formula and Empirical formula. Molecular formula = (…

Q: What is the mass, in grams, of 9.49×1024 molecules of methanol (CH3OH)?

A: Please find the attached images for the answer

Q: Determine the molar mass of Al(NO3)3⋅9H2O.

Q: A bottle of Ibuprofen (C 13 H 18 O 2 ) contains 1.204 * 10 ^ 24 molecules. How many grams of…

A: Interpretation - To determine the grams of ibuprofen are contained in the bottle when a bottle of…

Q: Quinine is used to treat malaria and has a molar mass of 325g/mol. If the empirical formula is…

Q: A molecular formula expresses the number of each kind of atom in a molecule. For example, the…

A: Given: Mass of compound = 6.50 g Mass of CO2 = 9.53 g. Mass of H2O = 3.90 g. Molar mass of CO2 = 44…

Q: Imagine that all our balances displayed mass in units of slugs instead of grams. Would we still…

Q: Arrange the following in order of increasing mass: 1.06 mol SF4; 117 g CH4; 8.7 × 1023 molecules of…

A: The following compounds in order of increasing mass have to be arranged

Q: Formaldehyde has the formula CH2O. How many molecules are there in 0.55 g of formaldehyde?

A: The molecular formula of Formaldehyde is CH2O Hence molar mass of CH2O = Atomic mass of C X 1 +…

Q: Calculate the mass in grams of 1.91*1024 molecules of formaldehyde. The chemical formula for…

A: Mass = number of mols x molar mass Number of molecules in 1 mole = 6.0224 x 1023 Molar mass of CH2O…

Q: If the molar mass of the hydrocarbon C3H8 was determined to be 440.97 g/mol, what is the molecular…

Q: The empirical formula of quinine is C10H12NO. If its molar mass is 324.42 g/mol, what is its…

A: Empirical formula= C10H12NOEmpirical mass=(12.01×10+1.008×12+14.00+16.00)g…

Concept explainers

Mass Spectrometry

This process is an instrumental method in which a sample is changed to fast moving positive ions by electron bombardment. The charged particles vary due to their different mass to charge ratio and are estimated with the help of this difference. It is also called mass spectroscopy.

Question

Initial Mass of Lighter before experiment
22.24g
Final Mass of Lighter after experiment
22.01g
Mass of butane transferred to the
graduated cylinder
Volume of butane in graduated cylinder
0.23 g
100.0 mL
Atmospheric Pressure
755 mm Hg
Temperature of water and gas
22°C
K
Vapor Pressure of water at 22°C
19.8 mm Hg
Pressure of Dry gas
0.23 atm

Using the formula for butane, C4H10, the ACTUAL molar mass of butane.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Please see image
3) A small portion of gaseous gasoline (boiling point of gasoline: ~185 oF, it becomes gas at 212 oF) was then injected to mix with air in the container described in Question 2, according to air/fuel ratio (14.7:1 by mass). Consider 90% mass of gasoline is isooctane and the rest is ethanol (C2H6O), how much are isooctane and ethanol in moles added, respectively? With the amount of gasoline injected, what is new total pressure of the container? (Mass of air = 0.892 g, Volume of container = 1.00 L, presure of air = 1.00 atm) 4) In “the intake stroke”, the air/C8H18 gaseous mixture in Question 3 is transferred into the cylinder, where the piston reaches the bottom of the cylinder. Assume the gas mixture an ideal gas behavior, the temperature of cylinder is 212 oF, and the total pressure of gas mixture is 1.00 atm, Calculate moles of C8H18, O2 and the total moles of air/fuel mixture. (Please answer both questions)
3) A small portion of gaseous gasoline (boiling point of gasoline: ~185 oF, it becomes gas at 212 oF) was then injected to mix with air in the container described in Question 2, according to air/fuel ratio (14.7:1 by mass). Consider 90% mass of gasoline is isooctane and the rest is ethanol (C2H6O), how much are isooctane and ethanol in moles added, respectively? With the amount of gasoline injected, what is new total pressure of the container? (Mass of air = 0.892 g, Volume of container = 1.00 L, presure of air = 1.00 atm) 4) In “the intake stroke”, the air/C8H18 gaseous mixture in Question 3 is transferred into the cylinder, where the piston reaches the bottom of the cylinder. Assume the gas mixture an ideal gas behavior, the temperature of cylinder is 212 oF, and the total pressure of gas mixture is 1.00 atm, Calculate moles of C8H18, O2 and the total moles of air/fuel mixture.
Mass of A sample: 0.045g Vol. of gas collected: 45.38mL Barometric Pressure : 755 mmHg Height of water column in tube 12.45cm H₂0 23.5°C Temp Vapor Pressure H₂0 at 23.5% 21.7mmltg Determine the pressure of dry Hydrogen gas in mm Hg. B) Determine the mass so that reacted in this exp. () Determine the experimental value for the equivalent. mass of Al based on this data (Report 2 sig Fig) Exp. Equivalent Mass of Al:
Give me handwritten answer with explaination?
Give a clear explanation handwritten answer...
Combustible vapor-air mixtures are flammable over a limited range of concentrations. The minimum volume % of vapor that gives a combustible mixture is called the lower flammable limit (LFL). Generally, the LFL is about half the stoichiometric mixture, the concentration required for complete combustion of the vapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL for n-hexane, C6H14. (b) What volume (in mL) of n-hexane (d 5 0.660 g/cm3) is required to produce a flammable mixture of hexane in 1.000 m3 of air at STP?
HPX Stude a ar-2903012.agilixbuzz.com/s... Ideal 110% Reset PAP Chemistry-2903012-4. Enriqs Solis O: SUBMISSION O OBJECTIVES Due: 4/ 5. How many moles of gas does it take to occupy 520 mL at a pressure of 400 torr and a temperature of 340 K? A. 0.0098 moles B. 0.0736 moles C. 73.6 moles D. 0.980 moles Works Cited VIEW GR
Chemistry 2. Calculate the Vm of Ar(g) at 200 K and I atm. B = -47 cm'/mol,.
Please see image
Composition of Dry Air at Sea Level Gas Mole% N2 78.084 O2 20.946 Ar 0.934 CO2 0.0345 Ne 0.00182 He 0.000524 CH4 0.000168 Kr 0.000114 a) Using data from the above table, calculate the partial pressure of Ar when the atmospheric pressure is 1.07 atm. b)
Pls help with part d