Derive a gas law formula for a specific scenario One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 F The temperature is then increased to 311K, but the container does not expand. What will the new pressure be? Part A The most appropriate formula for solving this problem includes only which variables? Enter the required variables, separated by commas (e.g., P,V, T). > View Available Hint(s)

Derive a gas law formula for a specific scenario One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 F The temperature is then increased to 311K, but the container does not expand. What will the new pressure be? Part A The most appropriate formula for solving this problem includes only which variables? Enter the required variables, separated by commas (e.g., P,V, T). > View Available Hint(s)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. An ideal gas is contained in a cylinder with a volume of 5.0x102 mL at a temperature of 30.0°C and a pressure of 710. torr. The gas is then compressed to a volume of 25 mL, and the temperature is raised to 820.0°C. What is the new pressure of the gas? 4. Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN3) to decompose explosively according to the following reaction: 2NaN3(s) 2Na(s) + 3N,(g) What mass of NaN3(s) must be reacted to inflate an air bag to 70.0L at 25°C and 0.995atm?
provide answer with full explanation ( only type )
I need help with part A and B
Pls help me with the following asap and make sure its 100% correct, thanks
[20.100] Gold exists in two common positive oxidation states, +1 and +3. The standard reduction potentials for these oxida- tion states are Au*(aq) + e Au(s) Eed = +1.69 V > Au*(ag) + 3 e → Au(s) Ered = +1.50 V (a) Can you use these data to explain why gold does not tar- nish in the air? (b) Suggest several substances that should be strong enough oxidizing agents to oxidize gold metal. (c) Miners obtain gold by soaking gold-containing ores in an aqueous solution of sodium cyanide. A very soluble com- plex ion of gold forms in the aqueous solution because of the redox reaction 4 Au(s) + 8 NaCN(aq) + 2 H,O(1) + O2(g) 4 Na[Au(CN),](aq) + 4 NaOH(aq) > What is being oxidized and what is being reduced in this reac- tion? (d) Gold miners then react the basic aqueous product solution from part (c) with Zn dust to get gold metal. Write a balanced redox reaction for this process. What is being oxi- dized, and what is being reduced?
Please do not round off sig figs in calculations until final answer. Thank you.
What are the units of a? What are the units of b? For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. atm Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 55.0 °C with a molar volume of 0.515 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm Explanation Check
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Hi, can someone please confirm if this would be the right answer, I'm not fully sure. Thank you!!
A 7.00 L tank at 19. °C is filled with 6.34 g of sulfur hexafluoride gas and 3.38 g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. sulfur hexafluoride carbon monoxide Explanation mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: Check U a atm atm atm 0 x10 X S 0/5 4 Letic Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
An unknown gas at 79.1 ∘C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what is the density of the gas? density: g/L
The combined gas law states that for a fixed amount of gas, the quantity PVIT is constant. This is often expressed by the equation PV1 PV2 T2 where P is the pressure, V is the volume, and T is the temperature, and the subscripts 1 and 2 denote two different conditions. Rearrange the combined gas law to solve for T2. T2 = A gas with an initial pressure of 1.42 atm, an initial temperature of 223 K, and an initial volume of 14.1 L is heated. The final pressure of the gas is 4.44 atm and the final volume of the gas is 11.2 L. What is the final temperature (T2) of the gas? T, = K