I have just moved and transferred to a new school. My chemistry class is really ahead of my old class, so I am having some problems that I just cannot understand through the book. I guess I could ask the teacher but I am a bit shy and this assignment is due Tuesday anyway. We are doing the gas laws and it is temperature-volume that I really cannot understand. If someone could show me how to do some of these problems it would help me. Just please don't give me the answers only because it will not help me on the upcoming test.. (Eeek!)
1. What would happen to a balloon's volume, originally at 20 degrees C, if you took the balloon outdoors in a temperature of 40 degrees C? Assume that the pressure is constant and the balloon does not allow any gas to escape.
2. In planning to administer a gaseous anesthetic to a patient,
a. Why must the anesthesiologist take into account the fact that during surgery the gaseous anesthetic is used both at room (18 degrees C) and the patient's body temperature (37 degrees C)?
b. What problems might arise if the anesthesiologist did not allow for the patient's higher body temperature?
3. An air bubble trapped in bread dough at room temperature (291K) has a volume of 1.0 mL. The bread bakes in the oven at 623K (350 degrees C):
a.Predict whether the air-bubble volume will increase or decrease as the bread bakes. Explain using the kinetic molecular theory.
b. Calculate the new volume of the air-bubble, using Charles' law.
4. You buy a 3.0-L helium balloon in a mall and place it in a car sitting in the summer sunlight. The temperature in the air-conditioned mall is 22 degrees C and the temperature in the the closed car is 45 degrees C
a. What will you observe happening to the balloon as it sits in the warm car?
b. What will be the new volume of the balloon?
If someone could help me out I would be really grateful. I noticed some of these questions looked alike so there must be something I could learn to be able to do it. It also might help if I actually knew what the kinetic molecular theory was..
Not all of these problems are work alike. It would have helped if you had told us what you didn't understand about them. In general, T goes up, V goes up. T goes down, V goes down. Remember this general equation.
(P1V1)/T1 = (P2V2)/T2
If its a Pressure, temperature problem, jut cross V1 and V2 out and work from there. If it's a pressure volume problem, just cross out T and work from there. ETC. Remember T is in Kelvin.
For problem 1.
1. What would happen to a balloon's volume, originally at 20 degrees C, if you took the balloon outdoors in a temperature of 40 degrees C? Assume that the pressure is constant and the balloon does not allow any gas to escape.
The problem isn't asking you to calculate anything. T was 20 and you take the balloon outside where it is 40. So T goes up, Volume goes up. So the answer is that the volume will increase.
3. An air bubble trapped in bread dough at room temperature (291K) has a volume of 1.0 mL. The bread bakes in the oven at 623K (350 degrees C):
a.Predict whether the air-bubble volume will increase or decrease as the bread bakes. Explain using the kinetic molecular theory.
KMT generally says that higher temperature causes the molecules/atoms to move faster which gives them more energy and they exert more pressure which will require that the air bubble become larger. I suggest you read in yur book about KMT. I can't type all that material here.
b. Calculate the new volume of the air-bubble, using Charles' law.
In my first post I said
(P1V1)/T1 = (P2V2)/T2. Notice that the pressure is constant; therefore, we just drop the P1 and P2 to arrive at
V1/T1 = V2/T2 and that is Charles' Law.
V1 = 1.0 mL
T1 = 291K
V2 = ?? solve for this
T2 = 623 K.
Solve for V2. I went through it and I have an answer of 2.14 which I would round to 2.1 mL.
This should get you started. Post again if you still have trouble but show us your work and/OR tell us exactly what you don't understand about the problem.
Also, I suggest one problem per post.
2. In planning to administer a gaseous anesthetic to a patient,
a. Why must the anesthesiologist take into account the fact that during surgery the gaseous anesthetic is used both at room (18 degrees C) and the patient's body temperature (37 degrees C)?
b. What problems might arise if the anesthesiologist did not allow for the patient's higher body temperature?
a.) Core temperature monitoring is used to monitor intraoperative hypothermia, prevent overheating, and facilitate detection of malignant hyperthermia.
I understand your concerns and I'd be happy to help you understand the concepts of temperature-volume relationships in the context of gas laws. Rather than directly providing you with the answers to these questions, I'll explain the key concepts and guide you through the process of solving them.
First, let's start with the basics. The kinetic molecular theory states that gases consist of particles (atoms or molecules) in constant random motion. The behavior of gases can be described and predicted using various gas laws, including Charles' Law and the ideal gas law.
1. Question: What would happen to a balloon's volume, originally at 20 degrees C, if you took the balloon outdoors in a temperature of 40 degrees C? Assume that the pressure is constant and the balloon does not allow any gas to escape.
To solve this question, we can use Charles' Law, which states that at constant pressure, the volume of a gas is directly proportional to its temperature. In equation form, it is V1 / T1 = V2 / T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.
Since the pressure is constant (as stated in the question), we can use Charles' Law to solve the problem. Let's assign values to the variables: V1 = initial volume = unknown, T1 = initial temperature = 20 degrees C = 293K, V2 = final volume = unknown, and T2 = final temperature = 40 degrees C = 313K.
Using the equation V1 / T1 = V2 / T2, we can rearrange it to V2 = V1 * (T2 / T1). Substitute the given values into the equation to find V2.
2. Question (a): Why must the anesthesiologist take into account the fact that during surgery the gaseous anesthetic is used both at room (18 degrees C) and the patient's body temperature (37 degrees C)?
The anesthesiologist needs to consider both room temperature and the patient's body temperature because the gas laws, particularly Charles' Law, state that the volume of a gas is directly proportional to its temperature. Since the anesthetic gas will go from a lower temperature (room temperature) to a higher temperature (the patient's body temperature), there will be an increase in volume if all other conditions remain constant.
Question (b): What problems might arise if the anesthesiologist did not allow for the patient's higher body temperature?
If the anesthesiologist did not account for the patient's higher body temperature, it could lead to an incorrect dosage of the anesthetic gas. This could potentially cause insufficient anesthesia, which may result in the patient experiencing pain or discomfort during the procedure.
3. Question (a): Predict whether the air-bubble volume will increase or decrease as the bread bakes. Explain using the kinetic molecular theory.
According to the kinetic molecular theory, as temperature increases, the average kinetic energy of gas particles also increases. This means the particles move faster and collide more frequently with each other and the walls of the container. Consequently, the increased collisions lead to an expansion of gases and an increase in volume. Therefore, as the bread bakes at a higher temperature, the air bubble's volume will increase.
Question (b): Calculate the new volume of the air-bubble, using Charles' Law.
To calculate the new volume of the air bubble, we can use Charles' Law. The equation is V1 / T1 = V2 / T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.
Given values are: V1 = 1.0 mL, T1 = 291K (room temperature), T2 = 623K (oven temperature).
Using the equation V1 / T1 = V2 / T2, rearrange it to V2 = V1 * (T2 / T1). Substitute the given values and calculate to find V2.
4. Question (a): What will you observe happening to the balloon as it sits in the warm car?
As the temperature of the air inside the balloon increases due to the warm car's temperature, the gas particles inside the balloon will gain more kinetic energy. This leads to faster particle movement and increased collisions with the walls of the balloon. As a result, the balloon will expand and appear larger.
Question (b): What will be the new volume of the balloon?
To calculate the new volume of the balloon, we can again use Charles' Law. The equation is V1 / T1 = V2 / T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.
Given values are: V1 = 3.0 L, T1 = 295K (22 degrees C), T2 = 318K (45 degrees C).
Using the equation V1 / T1 = V2 / T2, rearrange it to V2 = V1 * (T2 / T1). Substitute the given values and calculate to find V2.
By understanding the concepts of gas laws and using the equations provided, you can solve these problems on your own. If you encounter any specific difficulties or have further questions, feel free to ask!