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f 0.357 g of CHi gas is introduced into an evacuated 1.75 L flask at 25...
A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at...
A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol) Multiple Choice 18 Ο 776 g/mol Ο 144 g/mol Ο 66.1 g/mol Ο 739 g/mol Ο 81.4 g/mol
5.00 L flask is evacuated and 47.65 g of solid dinitrogen tetroxide, N204, is introduced at-196...
5.00 L flask is evacuated and 47.65 g of solid dinitrogen tetroxide, N204, is introduced at-196 ℃. The sample is then warmed to 25 °C during which time the N204 vaporizes and some of it dissociates to form brown NO2 gas. The pressure slowly increases until it stabilizes at 3.51 atm. a. Write the balanced reaction for the dissociation of N204 b. What would be the pressure in the flask at 25 °C if the gas were all N204? Number...
Consider the following equilibrium system: PCl5(g) -->PCl3(g) + Cl2(g) A 10.00 L evacuated flask is filled...
Consider the following equilibrium system: PCl5(g) -->PCl3(g) + Cl2(g) A 10.00 L evacuated flask is filled with 0.4334 mol PCl5(g) at 297.3 K. The temperature is then raised to 510.0 K, where the decomposition of PCl5 gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 2.665 atm. What is the value of the equilbrium constant in terms of concentrations, Kc, at 510.0 K?
A sample of gaseous PCs was introduced into an evacuated flask so that the pressure of...
A sample of gaseous PCs was introduced into an evacuated flask so that the pressure of pure PCI would be 0.48 atm at 433 K. However, PCIE decomposes to gaseous PCI; and Cly, and the actual pressure in the flask was found to be 0.80 atm. Calculate Ko for the decomposition reaction below at 433 K. PCI() = PCI;(9) + Cl2(0) Also calculate K at this temperature. At a particular temperature, 11.1 mol of SO3 is placed into a 3.8-L...
A flask with a volume of 1.02 L contains 14.58 g of an unknown gas at...
A flask with a volume of 1.02 L contains 14.58 g of an unknown gas at 35.1 °C and 846 torr. What is the molar mass of the unknown in g/mol? Report your answer to TWO places past the decimal. Do not include units. The gas constant R = 0.082058 L⋅atm/mol⋅K and 1 atm = 760 torr.
Carbon monoxide gas is collected at。°C ían evacuated flask with a measured volume or l 0.0...
Carbon monoxide gas is collected at。°C ían evacuated flask with a measured volume or l 0.0 L, when an the gas has been collected, the pressure in the flask is measured to be 0.410 atm Calculate the mass and number of moles of carbon monoxide gas that were collected. Be sure your answer has the correct number of significant digits mass: U +10 mole: mol
Fill in the Blanks Consider 1.75 g of an unknown gas. This gas is stored in...
Fill in the Blanks Consider 1.75 g of an unknown gas. This gas is stored in a 2.35 L flask at 53.0 °C and 1.05 atm The density of the gas B/L The molar mass of the gas g/mol
A pure solid sample of Substance X is put into an evacuated flask. The flask is...
A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a graph of the results: 190 150 temperature (°C) 110 heat added (kJ/mol Use this graph to answer the following questions: 150.0°C What is the boiling point of X? (check all that apply) solid liquid What phase (physical state) of X would you expect to find in the flask after...
Boron trifluoride gas is collected at -1.0 °C in an evacuated flask with a measured volume...
Boron trifluoride gas is collected at -1.0 °C in an evacuated flask with a measured volume of 25.0 L. When all the gas has been collected, the pressure in the Mask is measured to be 0.490 atm. Calculate the mass and number of moles of boron trifluoride gas that were collected. Round your answer to significant digits. mass: 0 mole: mol x 5 ?
Question 25 75.0 g of PCI,(g) is introduced into an evacuated 3.00 L vessel and allowed...
Question 25 75.0 g of PCI,(g) is introduced into an evacuated 3.00 L vessel and allowed to reach equilibrium at 250°C. PCI; (g) PCI; (g) + Cl (8) If K. = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? = 75.0 A) 2.88 atm 30.97+5(35.45 ) B) 2.27 atm = 0,360) mole C) 4.54 atm D) 7.42 atm E) 9.69 atm C HM 201/ Ghada El Zakhem Naous C= 0.360!=(0,120m N
A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol) Multiple Choice 18 Ο 776 g/mol Ο 144 g/mol Ο 66.1 g/mol Ο 739 g/mol Ο 81.4 g/mol
5.00 L flask is evacuated and 47.65 g of solid dinitrogen tetroxide, N204, is introduced at-196 ℃. The sample is then warmed to 25 °C during which time the N204 vaporizes and some of it dissociates to form brown NO2 gas. The pressure slowly increases until it stabilizes at 3.51 atm. a. Write the balanced reaction for the dissociation of N204 b. What would be the pressure in the flask at 25 °C if the gas were all N204? Number...
A sample of gaseous PCs was introduced into an evacuated flask so that the pressure of pure PCI would be 0.48 atm at 433 K. However, PCIE decomposes to gaseous PCI; and Cly, and the actual pressure in the flask was found to be 0.80 atm. Calculate Ko for the decomposition reaction below at 433 K. PCI() = PCI;(9) + Cl2(0) Also calculate K at this temperature. At a particular temperature, 11.1 mol of SO3 is placed into a 3.8-L...
Carbon monoxide gas is collected at。°C ían evacuated flask with a measured volume or l 0.0 L, when an the gas has been collected, the pressure in the flask is measured to be 0.410 atm Calculate the mass and number of moles of carbon monoxide gas that were collected. Be sure your answer has the correct number of significant digits mass: U +10 mole: mol
Fill in the Blanks Consider 1.75 g of an unknown gas. This gas is stored in a 2.35 L flask at 53.0 °C and 1.05 atm The density of the gas B/L The molar mass of the gas g/mol
A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a graph of the results: 190 150 temperature (°C) 110 heat added (kJ/mol Use this graph to answer the following questions: 150.0°C What is the boiling point of X? (check all that apply) solid liquid What phase (physical state) of X would you expect to find in the flask after...
Boron trifluoride gas is collected at -1.0 °C in an evacuated flask with a measured volume of 25.0 L. When all the gas has been collected, the pressure in the Mask is measured to be 0.490 atm. Calculate the mass and number of moles of boron trifluoride gas that were collected. Round your answer to significant digits. mass: 0 mole: mol x 5 ?
Question 25 75.0 g of PCI,(g) is introduced into an evacuated 3.00 L vessel and allowed to reach equilibrium at 250°C. PCI; (g) PCI; (g) + Cl (8) If K. = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? = 75.0 A) 2.88 atm 30.97+5(35.45 ) B) 2.27 atm = 0,360) mole C) 4.54 atm D) 7.42 atm E) 9.69 atm C HM 201/ Ghada El Zakhem Naous C= 0.360!=(0,120m N
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