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Boyle’s Law Example Problem
Boyle’s Law is a special case of the ideal gas law in which the pressure and volume of an ideal gas are inversely proportional to each other, providing the temperature and mass of the gas are held constant. Here’s an example of how to perform a calculation using Boyle’s Law.
Boyle’s Law Review
Pressure P and Volume V are inversely proportional when Temperature T and mass n are held constant:
P ∝ 1/V where V changes by a factor of z
P final = 1/z x V initial
Example Problem
For example, calculate the final volume of a gas if the pressure of a 4.0 L sample is changed from 2.5 atm to 5.0 atm.
You calculate z = P final /P initial z = 5.0 / 2.5 z = 2
P final = 1/z x V initial P final = 1/2 x 4.0 L P final = 2.0 L
Related Posts
Boyle's Law Explained With Example Problem
Volume's inversely proportional to pressure if temperature's constant
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Boyle's gas law states that the volume of a gas is inversely proportional to the pressure of the gas when the temperature is held constant. Anglo-Irish chemist Robert Boyle (1627–1691) discovered the law and for it he is considered the first modern chemist. This example problem uses Boyle's law to find the volume of gas when pressure changes.
Boyle's Law Example Problem
- A balloon with a volume of 2.0 L is filled with a gas at 3 atmospheres. If the pressure is reduced to 0.5 atmospheres without a change in temperature, what would be the volume of the balloon?
Since the temperature doesn't change, Boyle's law can be used. Boyle's gas law can be expressed as:
- P i V i = P f V f
- P i = initial pressure
- V i = initial volume
- P f = final pressure
- V f = final volume
To find the final volume, solve the equation for V f :
- V f = P i V i /P f
- V i = 2.0 L
- P i = 3 atm
- P f = 0.5 atm
- V f = (2.0 L) (3 atm) / (0.5 atm)
- V f = 6 L / 0.5 atm
- V f = 12 L
The volume of the balloon will expand to 12 L.
More Examples of Boyle's Law
As long as the temperature and number of moles of gas remain constant, Boyle's law means doubling the pressure of a gas halves its volume. Here are more examples of Boyle's law in action:
- When the plunger on a sealed syringe is pushed, the pressure increases and the volume decreases. Since the boiling point is dependent on pressure, you can use Boyle's law and a syringe to make water boil at room temperature.
- Deep-sea fish die when they're brought from the depths to the surface. The pressure decreases dramatically as they are raised, increasing the volume of gases in their blood and swim bladder. Essentially, the fish pop.
- The same principle applies to divers when they get "the bends." If a diver returns to the surface too quickly, dissolved gases in the blood expand and form bubbles, which can get stuck in capillaries and organs.
- If you blow bubbles underwater, they expand as they rise to the surface. One theory about why ships disappear in the Bermuda Triangle relates to Boyle's law. Gases released from the seafloor rise and expand so much that they essentially become a gigantic bubble by the time they reach the surface. Small boats fall into the "holes" and are engulfed by the sea.
Walsh C., E. Stride, U. Cheema, and N. Ovenden. " A combined three-dimensional in vitro–in silico approach to modelling bubble dynamics in decompression sickness ." Journal of the Royal Society Interface , vol. 14, no. 137, 2017, pp. 20170653, doi:10.1098/rsif.2017.0653
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(a) pressure/moles (b) temperature/volume (c) pressure/volume (d) temperature/moles (e) volume/moles
(a) pressure/temperature (b) pressure/volume (c) volume/temperature (d) moles/pressure (e) none of these
- What do you predict the volume will be when the pressure changes to 4.00?
- Sketch the completed pressure-volume graph.
- Click on " Effect of changing pressure on volume ." Describe what is added to the piston to increase the pressure.
- Sketch the completed volume-pressure graph.
- Write the formula equation for Boyle's Law.
- Write the equation for Boyle's Law in words.
- In the Animated Gas Lab , what are the units of pressure? (Click on Boyle's Law if you need help.)
- What are the units of volume used in this lab?
- Predict what the volume in this lab would be if the pressure were 8.00.
- Predict what the volume in this lab would be if the pressure were 0.500.
- State Boyle's law in your own words.
- Zip a sandwich bag nearly closed. Insert a straw into the opening and blow through the straw to inflate the bag so that it is a little over half full of air. Completely seal the bag. Now slowly roll the zipper part of the bag toward the bottom of the bag, decreasing the volume of the bag. Describe what happens to the pressure of the air in the bag as you decrease its volume.
- How does your experience with the plastic bag compare to the animated gas lab?
- If, in either situation, instead of having a closed container you had a small opening in the bottom of it, what would eventually happen to the gas?
- Referring to the previous question, what would happen to the volume of the gas in the container?
- Referring to the previous question, what would happen to the pressure of the gas?
- Based on the questions above, hypothesize why a rocket nozzle must constantly have gas flowing through it in order to maintain pressure.
ACTIVITY 2: PROBLEM SOLVING USING BOYLE'S LAW Sample Problem: A balloon with a vollume of 2.0 L is filled with a gas at 3 atmospheres. If the pressure is of the balloon? reduced to 0.5 atmospheres without a change in temperature, what would be the volume Since the fempevature doesn't change, Boyle's law can be used. Boyle's gas law can be expressed as: P_VV_1=P_1V_2 Giver: V_2=2.0 P_1=3 dtm P_2=0.5 otm Solution: P_1V_1=P_1V_2 V_2=P_1V_1PP_2 V_2=(200 ) atpa/ (0.5 alng)= V_2=6 I 0.5 V_2=12 L
Expert verified solution.
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problem to be solved and to be checked using boyle's law equation: In a J-shaped tube filled with mercury,initially, mercury levels in both limbs are the same.The initial volume of the trapped gas in the closed end is 0.50 L.The volume of the gas decreases to 0.30 L after the addition of mercury from the open end of the tube.
Boyle's law is a gas law which states that the pressure exerted by a gas (of a given mass, kept at a constant temperature) is inversely proportional to the v...
However, at high pressures or low temperatures, real gases may deviate from the ideal gas behavior described by Boyle's Law. Summary. Boyle's Law explains the inverse relationship between the pressure and volume of a gas, assuming constant temperature and gas amount. It is expressed mathematically as P 1 V 1 = P 2 V 2 . Understanding Boyle's ...
A gas occupies 4.31 liters at a pressure of 0.755 atm. Determine the volume if the pressure is increased to 1.25 atm. 2,400 mL. 600.0 mL of a gas is at a pressure of 8.00 atm. What is the volume of the gas at 2.00 atm? Study with Quizlet and memorize flashcards containing terms like 8.20 L, 1.44 L, 0.520 L and more.
Let's solve a typical Boyle's law problem. Boyle's Law Problem Example. Suppose a gas has a volume of 3.0 liters at a pressure of 2.0 atmospheres. If the pressure is increased to 4.0 atmospheres, what will the new volume of the gas be, assuming temperature remains constant? Solution: Write down the known quantities: V1 = 3.0 L, P1 = 2.0 atm, P2 ...
Boyle's Law is a fundamental concept in physics, specifically in the thermodynamics branch. It states that the volume (V) of a given amount of gas held at a constant temperature is inversely proportional to the pressure (P). In essence, if the volume increases, the pressure decreases and vice versa.
Boyle's Law describes the relationship between pressure and volume of a gas when mass and temperature are held constant. (NASA) Example Problem. For example, calculate the final volume of a gas if the pressure of a 4.0 L sample is changed from 2.5 atm to 5.0 atm. You calculate z = P final /P initial. z = 5.0 / 2.5. z = 2.
Boyle's gas law states that the volume of a gas is inversely proportional to the pressure of the gas when the temperature is held constant. Anglo-Irish chemist Robert Boyle (1627-1691) discovered the law and for it he is considered the first modern chemist. This example problem uses Boyle's law to find the volume of gas when pressure changes.
Figure 13.7.1: Boyle's Law. A piston having a certain pressure and volume (left piston) will have half the volume when its pressure is twice as much (right piston). One can also plot P versus V for a given amount of gas at a certain temperature; such a plot will look like the graph on the right. Boyle's Law is an example of a second type of ...
Step 1: Identify Boyle's Gas Law as P 1 V 1 = P 2 V 2 . Step 2: Plug in the known values of Pressure and Volume. Step 3: Rearrange the equation to isolate the unknown value. Step 4: Solve for the ...
However, we know something not in the problem: at sea level, the boiling point of water is 100 °C. So: 1) Let us use a ratio and proportion to estimate the pressure required for water to boil at 88 °C: 100 °C is to 101.3 kPa as 88 °C is to x x = 89.144 kPa. 2) Now, we can solve the problem using Boyle's Law: P 1 V 1 = P 2 V 2
Figure 11.4.1 11.4. 1: Boyle's Law. A piston having a certain pressure and volume (left piston) will have half the volume when its pressure is twice as much (right piston). One can also plot P versus V for a given amount of gas at a certain temperature; such a plot will look like the graph on the right. Boyle's Law is an example of a second ...
Problem #16: 4.00 L of a gas are under a pressure of 6.00 atm. What is the volume of the gas at 2.00 atm? Problem #17: A gas occupies 25.3 mL at a pressure of 790.5 mmHg. Determine the volume if the pressure is reduced to 0.804 atm. Problem #18: A sample of gas has a volume of 12.0 L and a pressure of 1.00 atm.
State Boyle's law in your own words. Zip a sandwich bag nearly closed. Insert a straw into the opening and blow through the straw to inflate the bag so that it is a little over half full of air. Completely seal the bag. Now slowly roll the zipper part of the bag toward the bottom of the bag, decreasing the volume of the bag.
To effectively tackle Boyle's Law practice problems, follow these step-by-step guidelines: 1. Familiarize yourself with Boyle's Law equation: Boyle's Law is expressed as P1V1 = P2V2, where P1 and V1 represent the initial pressure and volume of a gas respectively, and P2 and V2 represent the final pressure and volume. 2.
To find the final volume of the gas, we can use Boyle's law. Plugging in the given values and solving for the final volume, we find that it is 0.772 Liters. Explanation: To solve this problem, we can use Boyle's law, which states that the pressure and volume of a gas are inversely proportional at a constant temperature.
ACTIVITY 2: PROBLEM SOLVING USING BOYLE'S LAW Sample Problem: A balloon with a vollume of 2.0 L is filled with a gas at 3 atmospheres. If the pressure is of the balloon? reduced to 0.5 atmospheres without a change in temperature, what would be the volume Since the fempevature doesn't change, Boyle's law can be used.
Activity 2- Boyle's Law - Free download as Word Doc (.doc / .docx), PDF File (.pdf), Text File (.txt) or read online for free. Boyle's law activity
Activity No: 1 Table and Graph Analysis for Boyles Law Objectives: 1. State Boyle's Law. ... State Boyle's Law. Problem Solving 1. If 50 mL of a gas at 750 mmHg expands to 120 mL, what would be its new pressure? 2. A pressure of a gas of 95 kPa has a volume of 415 mL. What is the volume of the gas at 110 kPa? ... Get the Brainly App
To solve problems using Boyle's Law, the mathematical equation used is P1V1 = P2V2. Explanation: Boyle's Law relates the pressure and volume of a gas at constant temperature. The mathematical equation used to solve problems using Boyle's Law is P1V1 = P2V2. This equation states that the initial pressure multiplied by the initial volume is equal ...
When the pressure increases, the volume of the gas decreases. In the activity, as the volume of the syringe decreases, the pressure inside the syringe increases. You will expect an increased in pressure if you pushed the plunger of the syringe to lower the volume of the gas. The formula of Boyle's Law is P₁V₁ = P₂V₂.