How would you answer the second question? 12.25 13.SData Table:Analysis:1.2.3.4.5.6.7.corr rect temperature.Repeat this process for a second and third trial. Use a different lighter for each trial.The next day, find and record the mass of each of the butane lighters to the nearest 0.1mg.Trial numberlighter numberinitial mass of lighterfinal mass of lighter(we'll get this after they have dried overnight)Temperature(read from thermometer)volume of butane(read from eudiometer tube)Barometric pressure(read from barometer)vapor pressure of water(read from chart of vapor pressures)mm Hg.and record the vapor pressure of water in mm113.3509913.2482022.4°C14482mL29.85 inlig20.4523Convert the barometric pressure from inHg to mmHg. (1 in = 25.4 mm)Use Dalton's Law to calculate pressure of the butane alone.Using the Ideal Gas Law, calculate the moles of butane for each trial using the ideal gaslaw.11220.60gkrmol KPC141 molge = massmassVT7.07 96Calculate the mass of butane collected for each trial.Calculate the molar mass of butane gas for each trial.PVMolar Mass = Mass / # of molesCalculate the average molar mass of butane.Determine the formula of butane and the accepted molar mass of butane. Calculate the RTpercent error in your experimentally determined molar mass.PV=nRTIf some bubbles of butane escape and are not collected in the eudjometer, how will thehehar mass be affected? You would think the molarlorstod how will the

Second question :2. Given,Temperature = 22.4 °CBarometric pressure = 29.85 in HgVapor pressure of…

Answered: 1. 2. Use Dalton's Law to calculate…

1. 2. Use Dalton's Law to calculate pressure of the butane alone. Cac Law calculate the moles of butane for each trial using the

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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Question

How would you answer the second question?

12.
25 13.
S
Data Table:
Analysis:
1.
2.
3.
4.
5.
6.
7.
corr rect temperature.
Repeat this process for a second and third trial. Use a different lighter for each trial.
The next day, find and record the mass of each of the butane lighters to the nearest 0.1
mg.
Trial number
lighter number
initial mass of lighter
final mass of lighter
(we'll get this after they have dried overnight)
Temperature
(read from thermometer)
volume of butane
(read from eudiometer tube)
Barometric pressure
(read from barometer)
vapor pressure of water
(read from chart of vapor pressures)
mm Hg.
and record the vapor pressure of water in mm
1
13.35099
13.24820
22.4°C
14482mL
29.85 inlig
20.45
2
3
Convert the barometric pressure from inHg to mmHg. (1 in = 25.4 mm)
Use Dalton's Law to calculate pressure of the butane alone.
Using the Ideal Gas Law, calculate the moles of butane for each trial using the ideal gas
law.
11
220.60gkr
mol KPC14
1 molge = mass
mass
VT
7.07 96
Calculate the mass of butane collected for each trial.
Calculate the molar mass of butane gas for each trial.
PV
Molar Mass = Mass / # of moles
Calculate the average molar mass of butane.
Determine the formula of butane and the accepted molar mass of butane. Calculate the RT
percent error in your experimentally determined molar mass.
PV=nRT
If some bubbles of butane escape and are not collected in the eudjometer, how will the
he
har mass be affected? You would think the molar
lor
stod how will the

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