Constants PeriodicA neon sign is made of glass tubing whose inside diameter is2.5 cm and whose length is 5.5 m.Part AIf the sign contains neon at a pressure of 1.74 torr at 38 °C, how many grams of neon are in the sign? (The volume of a cylinder is πr²h.)Express your answer using two significant figures.3a54m =ΤΟ ΑΣΦSubmitRequest AnswerProvide Feedback%9o5MacBook Pro16&729?g8*(9ONext+ "

Given- Diameter• d = 2.5 cm r= d/2 = 2.5/2 = 1.25cmLength,• L = 5.5 m = 550 cm ( 1m =…

Answered: Constants Periodic A neon sign is made…

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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||| Understanding Boyle's Law A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 166. kPa. The piston is now pulled up, expanding the gas, until the gas has a final volume of 87.0 L. Calculate the final pressure of the gas. Round your answer to 3 significant digits. gas kPa piston Explanation cylinder @ 2 W Check 500 MA 3 X SO F3 E Ś $ 4 a R % 5 T 6 FA Y A 2 U 3/5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility DII -0 Danasia
Be sure to answer all parts. There are 7.69 × 1015 metric tons (T) of nitrogen in the atmosphere (1 metric ton = 1000 kg). How many short tons of nitrogen are present in the atmosphere (1 short ton = 2000 lb)?
Please answer the question and show your work. 6a. A helium balloon was partially filled with 8,000 ft3 (cubic feet or ft3, is a unit of volume) of helium gas when the atmospheric pressure was 0.98 atm and the temperature was 23 °C. The balloon rose to an altitude where the atmospheric pressure was 400 mm Hg and the temperature was 5.3 °C. What volume in ft3 did the helium gas occupy at this altitude?
please answer the question and show your work 5a. An automobile airbag inflates when sodium azide (NaN3) is converted to sodium (Na) and N2 gas according to the BALANCED equation, 2 NaN3 → 2 Na + 3 N2. What volume in liters (L) of N2 gas will be produced if 115 g of NaN3 completely reacted at STP (standard temperature and pressure). Molar mass of NaN3 = 65.02 g/mol 1 mol of any gas at STP = 22.4 L
Hydrogen gas has a density of 0.090 g/L, and at normal pressure and - 2.78 °C one mole of it takes up 22.4 L. How would you calculate the moles in 990. g of hydrogen gas? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles = x10 degreenobox
2. A 0.158-g sample of unknown metal, X, reacted with hydrochloric acid according the following (balanced) reaction: 2 X (s) + 6HCl(aq) → 2 XCl3 (aq) + 3 H₂ (g) The volume of hydrogen gas collected over water was 216 mL at 22 °C and a barometer reading of 764 mm Hg (VP of water at 22 °C is 20. mm Hg). SHOW ALL WORK. Find moles of (dry) hydrogen gas collected using PV=nRT, where R is 0.08206 L atm/mol K: Moles of hydrogen present Determine moles of "X" that would have been present initially to produce those moles of hydrogen using the mole ratio in the balanced equation above: Moles of metal present Determine the molar mass of "X" knowing that molar mass is grams per mole. 136 Atomic Mass of metal Identity of Unknown Metal
What is STP? standard theoretical measurements standard values for temperature and pressure O symbols of pure compounds standard technologies used in experiments
Use the reaction below for the combustion of ammonia gas to produce nitrogen monoxide and water vapor. 4NH3(9) + 302(g) What volume of O, is needed to react fully with 720 mL of NH3? → 4NO(g) + 6H»O(g)
A helium-filled balloon is launched when the temperature at ground level is 27.8°C and the barometer reads 752 mmHg. If the balloon's volume at launch is 9.47 × 10^{4}4 L, what is the volume in Liters at a height of 36 km, where the pressure is 73.0 mm Hg and temperature is 235.0 K? (Enter your answer using either standard or scientific notation. For scientific notation, 6.02 x 10^{23}23 is written as 6.02E23.)
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Use correct number of significant figures. 1. A gas at constant temperature with a volume of 895.0mls and pressure of 750.0 torr has the pressure increased to 850.0 torr. What is its new volume in Liters? 2. At what temperature in °C does 0.505 moles of gas occupy a volume of 8.15 Liters at a pressure of 0.750 atm? 3. a) How many moles of Cl2 gas occupy a volume of 695 mL at 6.40 atm and 337 Kelvin? b. How many grams of Cl2 gas are present? 4. A gas at constant pressure occupies a volume of 200.0 mL at 27.0°C . At what temperature in °C would the volume be 280.0mL ?
According to Avogadro's law, how will the number of molecules in 2 liters of hydrogen gas compare with the number of molecules in 2 liters of oxygen gas at the same temperature and pressure? Answer in a complete sentence. H + Normal Enter your answer here **** √x = 201 BIUS X₂ X² EEAA

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