Gas Laws Lab


The 4 standard physical homes of a gas sample are pressure, volume, temperature level, and variety of moles. The volume merely shows the volume of the container because a gas will take up all area offered to it. The temperature level shows the average kinetic energy of the gas particles. For gases, the temperature needs to be converted to the Kelvin system. The pressure of the gas shows the variety of collisions with each other and the wall of the container.

The number of moles suggests the amount of gas particles.

Gases do not have a certain shape of volume. Gases spread out into their container and inhabit the entire volume readily available, which means they are totally free to move and have big amounts of empty space. In many chain reactions, gases are produced; for instance, reactions including metal carbonates that respond with an acid produce gaseous co2. Objective:

To figure out the volume of gas produced from a response between a metal carbonate and acid and to identify the identity of an unidentified carbonate salt.

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Pre-Lab Questions:
1. If you increase the temperature level what takes place to the speed of the particles? Explain. 2. What is the formula to convert Celsius temperature level to Kelvin? a. ° C +273.15= K.
3. What are the basic conditions for a gas? Are you at standard conditions in the lab? 4. Boyle’s Law – The principle that the volume of a provided mass of an ideal gas is inversely proportional to its pressure, as long as temperature level remains continuous.

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Boyle’s law is a subcase of the ideal gas law. P1V1 = P2V2 Charles’ Law– The law of volumes. The volume of a repaired quantity of gas at continuous pressure is directly proportional to the Kelvin temperature level of the gas. (Temperature must be in Kelvin). V1T1= V2T2 V/T = K V1T2 = V2T1 Gay-Lussac’s Law– Pressure is straight proportional to temperature if the volume is continuous. P1/T1 = P2/T2 5. What is the Perfect Gas Law in formula type? What is the value for the proportionality constant with units? Why are those systems so crucial?
b. PV = nRT
c. C = PV / T
6. Write the balanced equations for CaCO3, BaCO3, Li2CO3, and Na2CO3 reactions with hydrochloric acid. 7. Calculate the molar mass of these same four metallic carbonates. LiCo3 = mass/mole; 3.0036g/0.0344 mol = 87.31 g/mol

* 3.0 M HCl (aq)
* 5 ml graduated cylinder
* Balloon String
* Scissors
* Weighing paper
* 3g of unknown #2 carbonate salt
* Funnel

First measure out 5ml of 3.0 M HCl into the graduated cylinder and weigh 3 g of the unknown carbonate salt. Using the funnel, pour the unknown carbonate salt into the balloon and put the open end of the balloon over the graduated cylinder and secure with a string. It is important to make sure the string is very tight to prevent the gas from leaking. Empty the contents of the balloon into the graduated cylinder that contains the 3.0 M HCl. After the gas fills the balloon, use a string and measure the circumference of the balloon.| Observations:Carbonate is limiting reactant.|

Based upon our experiment, equations, and calculations that our unknown Carbonate Salt for Unknown # D was Li2CO3 – Lithium Carbonate. There could be a number of factors that could have caused us to receive an 18.1% error. How we held the balloon when tipping it over the acid could greatly affect the radius of our balloon.

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Gas Laws Lab. (2016, Dec 14). Retrieved from

Gas Laws Lab

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