M Here is a graph of the probability of an atom moving with a particular speed, for a sample of xenon gas at -55. °C. probability 100 200 speed (m/s) What is the most likely speed of a Xe atom in this sample? Use this graph to answer the following questions. Round each of your answers to the nearest m/s. Note: your answers must be within 25 m/s of the exact answers to be graded correct. What higher speed is only half as likely as the most likely speed? 300 What higher speed is only 10% as likely as the most likely speed? e O 400 E B B Ew

M Here is a graph of the probability of an atom moving with a particular speed, for a sample of xenon gas at -55. °C. probability 100 200 speed (m/s) What is the most likely speed of a Xe atom in this sample? Use this graph to answer the following questions. Round each of your answers to the nearest m/s. Note: your answers must be within 25 m/s of the exact answers to be graded correct. What higher speed is only half as likely as the most likely speed? 300 What higher speed is only 10% as likely as the most likely speed? e O 400 E B B Ew

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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ut Cambria 14 A A Aa - AaBbC Ppy - a - A - T Norm BIU abc x, x prmat Painter ard Font Paragraph A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of gas. The gas was collected by water displacement in a 22°C water bath. The barometric pressure in the lab that day was 746 mmHg. A. Using Dalton's Law and the vapor pressure of water at the given temperature to calculate the partial pressure of hydrogen gas in the collection tube. B. Use the combined gas law to calculate the corrected volume of hydrogen at STP. I C. What is the theoretical number of moles of hydrogen that cạn be produced from 0.028 g of magnesium reacting with excess hydrochloric acid? D. Divide the corrected volume of hydrogen gas by the theoretical number of moles of hydrogen to calculate the molar volume of hydrogen at STP. 1302 words Type here to search 近

To derive the ideal gas equation, we assume that the volume of the gas atoms or molecules can be neglected.
18) What will the temperature of a 2100. mL sample of nitrogen at 526. mm Hg and 42.4oC be, in oC, after it changes to 1290. mm Hg and 3100. mL? Put your answer with 3 significant digits.
1. Natural gas reforming produces hydrogen gas from methane. In this reaction methane (CH4) gas reacts with high temperature steam (boiling water) to form hydrogen gas and carbon monoxide. a. Write a balanced equation describing what happens. b. Calculate the atom economy for the production of hydrogen gas using this reaction. c. 5.0 grams of methane undergoes this reaction in a 15.0 L container at 125 °C, what is the final pressure of the hydrogen gas produced by the reaction.
Here is a graph of the probability of an atom moving with a particular speed, for a sample of xenon gas at -141. °C. ^ 100 200 speed (m/s) probability Use this graph to answer the following questions. Round each of your answers to the nearest m/s. Note: your answers must be within 25 m/s of the exact answers to be graded correct. What is the most likely speed of a Xe atom in this sample? What higher speed is only half as likely as the most likely speed? What higher speed is only 10% as likely as the most likely speed? 300 X 0 0²
Argon diffuses at a rate of 1.45 meters in 8.65 minutes. How long will it take helium to diffuse 5.86 meters under the same conditions? (I should see the calculation of rates first.)
At what temperature (in degrees Celsius) will xenon atoms have the same average speed that Br2 molecules have at 45∘C?
Since volume and pressure are inversely related, we can make some assumptions about initial and final states using the data provided. We can also identify initial and final states by finding trigger words in the language of the problem. Look for words like “first,” “initially,” or “originally” to describe initial states and “result” or “after” for final states. What volume would a sample of helium occupy at 6.0 atm if the helium was initially compressed in a 1.0 L tank at 20. atm at constant temperature? Organize your data into the table to help analyze the problem. Leave blank any boxes for which you do not have information. Drag the appropriate labels to their respective targets.
Ammonia Production Ammonia is often formed by reacting nitrogen and hydrogen gases. How many liters of ammonia gas can be formed from 13.7 L of hydrogen gas at 93.0°C and a pressure of 40.0 kPa?
Part B The pressure in car tires is often measured in pounds per square inch (Ib/in.), with the recommended pressure being in the range of 25 to 45 lb/in.2. Suppose a tire has a pressure of 42.5 lb/in.? . Convert 42.5 lb/in.? to its equivalent in atmospheres. Express the pressure numerically in atmospheres. • View Available Hint(s) να ΑΣφ ? 42.5 lb/in.? : atm
4. Two students, Imani and Josiah, are discussing their results: Predicted volume: 75.7 ml Measured volume: 71.9 ml Imani says: (1) I think the gas is warmer than 23°C after the reaction. This means our conversion factor of 24 L is too low. There are more than 24 liters for every mole. Josiah says: (2) I think there is friction in the piston in the gas collection tube, which prevents it from moving all the way out. Which explanation matches their results? (Enter 1 or 2. Enter 3 if neither explanation is consistent with the results.)
A sample of polyatomic gas weighs 6.94 g and at a temperature 30.0 C it has a volume of 2.49 L and a pressure of 361 torr. What is the molecular weight of the gas? (hint: remember that PV=nRTPV=nRT) The molecular structure of the gas in the above problem has a total of 7 atoms and contains only sulfur and fluorine atoms. Based on its molecular weight you calculated above, which of the following empirical formulas is most likely to be correct for the gas? SF6 S2F5 S3F4 S4F3 S5F2 S6F None of these formulas are correct