SOLVE THE FOLLOWING PROBLEM USING BOYLE'S LAW EQUATION. VIP1 = V2P2 1. A 500 ml sample of hydrogen is collected when the pressure is 800 mmHg. What volume will the gas occupy when the pressure is 760 mmHg? 2. A 40 L balloon is filled with gas at 4 atm. What will be its new volume at standard pressure of 1 atm?

Q: The pressure on 2.50 L of anesthetic gas changes from 787.5 mmHg to 303.8 mmHg. What will be the new…

A: Ideal gas equation PV = nRT   P = Pressure V = Volume n = Moles R = Gas constant T = Temperature

Q: Part B Consider 4.90 L of a gas at 365 mmHg and 20 °C. If the container is compressed to 2.10 L and…

A: Part B4.90 L of a gas at 365 mm Hg and 20 °C, the container is compressed to 2.10 L and the…

Q: example in Part A has an initial volume of 42.0 L , and you have determined that it contains 1.60…

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Q: Question 12 Which of the following statements is true? O Each real gas deviates from ideal gas…

A: Answer: This question is based on van der walls equation of real gases which is shown below:…

Q: Use Charles's law to complete the table. (Assume pressure and number of moles of gas to be…

A: Charles's law  -                        Charles's Law states that the volume of a given mass of gas…

Q: final pressure

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Q: A sample of gas has a volume of 2.09 L at a temperature of 49.90 °C. The gas sample is cooled to a…

A: Given that, initial volume(v1) = 2.09  L, initial temperature(t1) = 49.90°C = (273 + 49.90)K = 322.9…

Q: Part A: Calculate the molar mass of a gas that has a density of 1.98 g/L at STP.   Part B:…

A: To Solve this problem we use the relation that   d = PM/RT  Where , d = density   P = pressure  M =…

Q: A sample of gas at 47°C and 1.03 atm occupies a volume of 2.20 L. What volume would this gas occupy…

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Q: A gaseous mixture consists of 6.91 g of N2, 4.71 g of O2, and 2.95 g of He. Determine the partial…

A: Given, 6.91 g of N2, 4.71 g of O2, and 2.95 g of He T = 28 degrees celsius P = 1.05 atm pressure

Q: When the ideas from Boyle’s Law, Charles’ Law and Gay-Lussac’s Law are combined, you get the…

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Q: - How many moles of vapor are there in a sample that completely fills a 125-mL flask at . 85.5°C and…

A: Given: Volume = 125 mL Temperature = 85.5oC Pressure = 763 torr

Q: 3. Calculate the decrease in temperature when 6.00 L at 20.0 °C is compressed to 4.00 L. (Chanes…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Use Charles's law to complete the table. (Assume pressure and number of moles of gas to be…

A:

Q: Q1. A hydrocarbon (Ma=224.253 g/mol) found to contain 64.27% carbon and 7.19% hydrogen by mass, the…

A: We will first determine the molecular formula of the organic compound. Then apply stoichiometry to…

Q: Avogadro's Law 1. a container with a volume of 25.47 L holds 1.050 mol of oxygen gas (O2) whose…

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Q: The product gas, O2, is collected over water at a temperature of 20 °C and a pressure of 741 mm Hg.…

A: Given: Vapor pressure of water = 17.5 mm Hg The total pressure of gas = 741 mm Hg Temperature = 20…

Q: 3. Complete this table 田 Gas Law Formula Variable Held Constant Charles V=kT V Вoyle Px=k K Avogadro…

A: Ideal gases are hypothetical gases that do have real existence. A gas can behave ideally at low…

Q: given problems as well. SHOW YOUR SOLUTION. 1. A balloon with a volume of 12.0 L is filled with a…

A: Initial volume of baloon = 2.00 L  Final Volume = ?  Initial pressure = 3.8 atm  Final pressure =…

Q: Using the Ideal Gas Law to Calculate Molar Mass A 1.22-g sample of an unknown gas has a volume of…

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Q: Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle’s Law is described…

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Q: Complete the fourth row of the table. Express the temperature in degrees Celsius to three…

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Q: Consider the apparatus shown below with the valve initially closed. The volume and pressure in each…

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Q: Use Charles's law to complete the table. (Assume pressure and number of moles of gas to be…

A: In this question we will use Charles law to complete the given table. Charles law states that for a…

Q: A sample of gas in a cylinder has an initial volume of 40.0L and it has 1.7 moles of gas. The next…

A: Avogadro’s law, is a gas law which states that the total number of atoms/molecules of a gas (i.e.…

Q: to a final temperature of 150 °C while the volume is held constant, what is the final pressure?…

A: Answer:- This question is answered by using the simple concept of gaseous laws which involves the…

Q: A mixture of SO3, SO2, and O2 has a total pressure of 4.42 atm. The partial pressure of SO3 is 1.77…

A: According to  Dalton's law  Total pressure of gas mixture is equal to the sum of partial pressure of…

Q: O 3.00 atm

A: Initial partial pressure of He = 1.5 atm Intial volume = 1.0 L Final Volume = 0.500 L At constant…

Q: Answer the 3 questions below 1. If a gas occupies 6.50 liters at 2oC, to what temperature, in…

A: 1. Given :             V1 = 6.50 L             V2 = 7.00 L               T1 = 200C = 293K We have to…

Q: 1. What is the value of the Clausius-Clapeyron Constant?

A: Since you asked multiple questions so as per Q&A guidelines of portal I solve first question…

Q: When the ideas from Boyle's Law, Charles' Law and Gay-Lussac's Law are combined, you get the…

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Q: The volume of a sample Chlorine gas (Cl2) is 6.80 L at 1200 torr and 41 °C. Calculate how…

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Q: Use Charles's law to complete the table. (Assume pressure and number of moles of gas to be…

A: Complete the first row of the table. Express the volume in litres to three significant figures.

Q: Use Boyle's law to complete the following table (assume temperature and number of moles of gas to be…

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Q: The pressure in a car tire is 28.7 psi at 27 °c. At the end of a trip on a hot day, the pressure has…

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.