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Question 4 How will the pressure change if a sample of an ideal gas in a...
How will the pressure change if a sample of an ideal gas in a rigid 2.0 L container initially at 250 °C is cooled to -142 °C? • The final pressure will be 1/4 of the original pressure. The final pressure will be 1/2 of the original pressure. The final pressure will be the same as the original pressure. The final pressure will be 4 times the original pressure. The gas pressure is reduced to zero The final pressure will...
4. Suppose we change the pressure of an ideal gas at constant temperature. How is the corresponding AG related to its AS for the same process? For example, are they proportional to each other, and - if so - what is the proportionality constant?
a. 242 m/s b. 1.21 x 103 m/s c. 822 m/s d. 483 m/s 25. Is this rms speed the same or different from the nitrogen molecules in the sample? Explain. 26. An ideal gas sample of 11 moles initially at STP is isothermally compressed to half its original volume. What must be its final pressure? a. 4.8 atm b. 3 atm c. 2 atm d. 4 atm 27. In the previous question, by what factor does the internal energy...
A sample of ideal gas at room temperature occupies a volume of 31.0 L at a pressure of 862 torr. If the pressure changes to 4310 torr, with no change in the temperature or moles of gas, what is the new volume, V2? Express your answer with the appropriate units. ► View Avallable Hint(s) V2 = 6.20 L Submit Previous Answers Correct Part B If the volume of the original sample in Part A (P1 - 862 torr. Vi =...
The temperature used in the ideal gas law must be expressed in a. Celsius b. Fahrenheit c. Kelvin d. Pascale e. Any of the above 680 Fahrenheit is equivalent to a. 273 Kelvin b. 298 Kelvin c. 0 Celsius d. 212° Fahrenheit e. None of the above Which has more mass, a mole of Nitrogen and a mole of Hydrogen a. 1. 2. 3. Nitroger b. Hydrogen c. Both have same mass d. Neither has any mass 4. Two identical...
Constants Part A A volume of air (assumed to be an ideal gas) is first cooled without changing its volume and then expanded without changing its pressure, as shown by the path abc in the figure (Figure 1). How does the final temperature of the gas compare with its initial temperature? Express your answer using two significant figures T1.0 T. Figure < 1011 > Previous Answers p (Pa) Correct 3.0 x 10 2.0 × 105 PartB 1.0 × 105 b...
Problems 1. According to the Ideal Gas Law, which of the following is/are correct for a gas cylinder of fixed volume filled with one mole of oxygen gas? Please explain each one. a. When the temperature of the cylinder changes from 15 °C to 30 °C, the pressure inside the cylinder doubles. b. When a second mole of oxygen is added to the cylinder, the ratio T/P remains constant. C. An identical cylinder filled with the same pressure of hydrogen...
Calculate molar volume of an ideal gas in m^3 at room temperature and pressure (or RTP). Id other words, calculate how much volume one mole of an ideal gas at 1.01 times 10^5 Pa and 298 K takes up. Then convert it to liters (l), where 1 t - 0.001 m^3 Measured at 18.00 C, a lead rod has a length of 52.44 cm, and an iron rod has a length of 52.61 cm. Both rods are heated to 86.0...
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QUESTION 3 4.(9 points) Consider 0.333 mL of an ideal gas initially at 44.00 °C in a sealed container. What is the final volume after the gas is heated to 100.00 °C at constant pressure? Report your answer in mL with three decimal places. QUESTION 4 7.(7 points) What is the total pressure of a gas mixture composed of 0.622 atm He gas, 844 torr Ne gas and 378 mmHg Ar gas? Report your answer in...
Question 1 (1 point) Calculate the density of nitrogen gas in a 4.32 L container at 1.0 atm and 25°C. Question 1 options: 0.57 g/L 0.74 g/L 1.15 g/L 1.31 g/L 1.56 g/L Save Question 2 (1 point) What volume is occupied by 1.00 kg of nitrogen gas at 5.00?C at a pressure of 735 Torr? Question 2 options: 1686 L 1242 L 843 L 738 L 621 L Save Question 3 (1 point) The ideal gas law fails to...