# GAS LAW and other PRE LAB HELP

• ANIMAL who
In summary, the Ideal Gas Law can be used to calculate the number of moles of gas at 1.00atm in a cell with a length of 10.0cm and a cross-sectional area of 1.00cm^2 at 298K. Additionally, if 374mL of a person's breath is needed to change the color of phenolphthalein from pink to colorless, the number of moles of CO_2 per L of breath (concentration of CO_2) can be calculated using the equation CO_2 + OH^- yields HCO^-_3.
ANIMAL who
#1-Use the Ideal Gas Law to calculate the number of moles of gas at 1.00atm in a cell 10.0cm long having a cross sectional area of 1.00cm^2 at 298K. (1ml=1cm^3)

#2-Lets say you start with 6.0 x 10^2 mL of 1.0 x 10^-4 M NaOH solution containing phenolphthalein indicator. The equation is CO_2 + OH^- yields HCO^-_3 (HCO bottom number of three with an overall negative charge) If 374 mL of a persons breath is required to turn the phenolphthalein from pink to colorless, calculate the number of moles of CO_2 per L of breath (ie., the concentration of CO_2) in this breath.

ANIMAL who said:
#1-Use the Ideal Gas Law to calculate the number of moles of gas at 1.00atm in a cell 10.0cm long having a cross sectional area of 1.00cm^2 at 298K. (1ml=1cm^3)

#2-Lets say you start with 6.0 x 10^2 mL of 1.0 x 10^-4 M NaOH solution containing phenolphthalein indicator. The equation is CO_2 + OH^- yields HCO^-_3 (HCO bottom number of three with an overall negative charge) If 374 mL of a persons breath is required to turn the phenolphthalein from pink to colorless, calculate the number of moles of CO_2 per L of breath (ie., the concentration of CO_2) in this breath.

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I would like to provide a response to the content regarding the Ideal Gas Law and the pre-lab help needed.

Firstly, to calculate the number of moles of gas at 1.00atm in a cell 10.0cm long with a cross-sectional area of 1.00cm^2 at 298K, we can use the Ideal Gas Law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. In this case, we are given the pressure (1.00atm), volume (10.0cm x 1.00cm^2 = 10.0cm^3 = 10.0mL), and temperature (298K). We can rearrange the equation to solve for n, which gives us n = PV/RT. Plugging in the values, we get n = (1.00atm x 10.0mL)/(0.0821 L atm/mol K x 298K) = 0.00425 moles of gas.

Moving on to the second part, we have been given a NaOH solution with a concentration of 1.0 x 10^-4 M and phenolphthalein indicator. The equation given is CO_2 + OH^- yields HCO^-_3, which suggests that CO_2 is reacting with OH^- to form HCO^-_3. The question asks us to calculate the number of moles of CO_2 per L of breath, which is essentially the concentration of CO_2 in the breath.

To find the concentration, we can use the formula C = n/V, where C is the concentration, n is the number of moles, and V is the volume. We have been given the volume of breath (374mL) and the number of moles of NaOH (6.0 x 10^2 mL x 1.0 x 10^-4 M = 0.06 moles). However, we need to convert the volume of breath from mL to L, which gives us 0.374L. Plugging in the values, we get C = 0.06 moles/0.374L = 0.16 M. This means that the concentration of CO_2 in the

## 1. What is the ideal gas law and how is it used in scientific experiments?

The ideal gas law, also known as the universal gas law, is a mathematical equation that describes the behavior of gases under various conditions. It states that the pressure, volume, and temperature of a gas are all directly proportional to each other. This law is commonly used in scientific experiments to predict the behavior of gases in different environments, and to calculate the properties of gases based on known variables.

## 2. What are the units of measurement for the variables in the ideal gas law?

The units of measurement for the variables in the ideal gas law are as follows: pressure is measured in atmospheres (atm), volume is measured in liters (L), and temperature is measured in Kelvin (K). It is important to use these units consistently in order to accurately apply the ideal gas law in experiments.

## 3. How does the ideal gas law differ from real gas behavior?

The ideal gas law assumes that gases behave in a perfectly ideal manner, meaning that they have no volume and do not interact with each other. In reality, gases do have a small amount of volume and do interact with each other, which can result in deviations from the ideal gas law at high pressures and low temperatures.

## 4. What is the purpose of a pre-lab in scientific experiments?

A pre-lab is an important step in the scientific method that involves planning and preparing for an experiment. It allows scientists to familiarize themselves with the experimental procedure, anticipate any potential issues or safety concerns, and ensure that they have all the necessary materials and equipment. Pre-labs also often involve background research and hypothesis formation to guide the experiment.

## 5. How can I ensure accurate results when using the ideal gas law in experiments?

To ensure accurate results when using the ideal gas law, it is important to carefully measure and record all variables, use appropriate units of measurement, and follow the correct formula. It is also important to consider any potential sources of error, such as leaks or temperature fluctuations, and take steps to minimize them. Additionally, repeating the experiment multiple times and taking an average of the results can help to reduce random errors and increase the accuracy of the data.

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