top-rated free essay

# Experiments and Error Analysis: Ideal Gas Law and the Molar Enthalpy of Vaporization

By bworb Dec 03, 2013 467 Words
﻿Discussion Section
In the experiment the main concepts were the ideal gas law, the molar enthalpy of vaporization (, and the.
Using the equation and the plotted graph we know that the slope is equal to , with the intercept C. With the plotted points of lnP and 1/T we can find the value. We also know that is independent of temperature as long as the temperature range is limited and the pressure is about 1 atm, which in our situation both are true.

A simple but key procedure that was made in the experiment was when the 10 ml beaker was inverted and put into the 1000ml beaker. This is important because this is when the air bubble was made sure to have the same pressure as the room and satisfy the equation.

When the 1000ml beaker containing the inverted 10 ml graduated cylinder with the air bubble was heated to about 80 degrees Celsius, the air bubble expanded due to the additional water vapor and the expansion of gas at higher temperatures.

Cooling the water in the 1000 ml beaker to about 5 degrees Celsius made it possible to find the number of moles of present air because the water vapor is negligible at this low of a temperature. Once the temperature of the water inside the 10 ml graduated cylinder has equilibrated with the water inside the 1000 ml beaker, the temperature and volume of the air bubble, along with the pressure in the air bubble which is equal to the pressure in the room of the can be used with the ideal gas law to find .

Error Analysis
The standard deviation of the slope of the best fit line was 116.83 of the -4747.76 slope value. The standard deviation of the y-intercept was 0.3458 of the 12.716 y-intercept value. The standard deviation the ΔHvap(water) was 0.9714 of the 39.475 ΔHvap(water) value. The percent deviation of the ΔHvap(water) from the reported literature value of 40.66kJ/mol was 4.0826%.

The 10ml graduated cylinder used had an uncertainty of +/-0.1ml. In the original measurement of water in the graduated cylinder of 8.75ml there would be a 1.14% uncertainty. The yellow digital thermometer had an uncertainty of +/-0.1 degrees Celsius. The thermometer is taking temperatures from 79.5 degrees Celsius to 3.1 degrees Celsius so the percent uncertainty would be anywhere from 0.126% to 3.23%.

In this experiment there were minimal experimental errors and uncertainties. Small errors and uncertainties like the 10 ml graduated cylinder not being flat on the bottom of the 1000ml beaker, leads to a slight misread of the volume but this is such a minimal error that the results would not be too skewed because of it.

The largest sources of error come from the standard deviation for the slope, y-intercept, and ΔHvap(water). Also from the equipment uncertainty of the 10ml graduated cylinder and the yellow digital thermometer. I hate chemistry.

## Related Documents

• ###### Ideal Gas Law

...Ideal Gas Law Packet Name ______________________________ 12.3 Date __________________ Period _______ Given: Ideal Gas Law = then P = n = V = T = R = 1. What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20.(C? 2. Oxygen gas is...

• ###### Ideal Gas Law

...Name of the Experiment: Avogadro’s Law Type Your Name: Date: 11/17/13 Experiment 1 ________________________________________ 1. For each gas, record the following: Propane Butane Methane a Name and formula C3H8 C4H10 CH4 b Mass of 100 mL gas (g) 0.274g 0.361g 0.100g c Molecular weight of the gas (g/...

• ###### Lab Report on Ideal Gas Law

...Ideal Gas Law Lab 1. Procedure: First, we used a balance to weigh the canister of gas, and recorded that mass as the original weight. Then, we filled a large bucket with water and recorded the temperature. We then filled a small test tube with water at the same temperature and poured that water into a graduated cylinder to measure the origina...

• ###### Discussion for Gas Law Experiment

...Chemistry I Gas Laws Gas Laws: Pressure, Volume, and Temperature Introduction Pressure, volume, and temperature are properties of gases that reveal their relationships when any one of them is varied. Changing the temperature of a gas may change its volume or pressure, but how? What are the mathematical relationships between these properties...

• ###### Ideal Gas Law and Magnesium

...Group : 1 Partner’s Name :Lam Meng Hui 1101920 Tan Boon Khai 1102510 Dang Zien Loong 1102446 Experiment Number : 8 Experiment Title :Determination of the valency of magnesium Date :29/6/2011 Lecturer :Dr Ha Sie Tiong Title: Determination of the Valency of Magnesium Objective To study the quantitative relationship b...

• ###### Molar mass of an ideal gas

...source. Part 2: Gas Tubes a.) I then moved to the gas tubes, starting with Helium. I placed myself at in front of the light tube & aimed the spectroscope for the center. b.) Repeated process with the remaining gases, Ne and Hg. Part 3: Flame Test a.) I turned the Bunsen burner to the desirable flame. b.) I then took the Bari...

• ###### Determining Molar Mass by Ideal Gas Law

...I. Abstract: By manipulating the ideal gas law (PV=nRT), we will be determining the molar mass of an unknown volatile liquid. Heating a flask filled with an unknown, easily evaporated liquid will allow for measurements that can be taken to work out the ideal gas equation. This lab will require knowledge of basic equations used in c...

• ###### Lab: How the Ideal Gas Law Applies to Real Physical Experiments

...﻿Student: Wanda Matison Rhodes Date: March 12, 2015 Partner: Tiara Key Section: 721 Introduction The objective of this lab was to examine how the Ideal Gas Law applies to real physical experiments. Using the Ideal Gas Law, we were able to find absolute zero and the universal gas constant. An ideal gas is a gas that is composed of a ...