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Question 22 (4 points) Saved A sample of air then may have 5.55 moles of N2...
Question 21 (4 points) Saved A sample of air has 3.55 moles of N2 and 2.50...
Question 21 (4 points) Saved A sample of air has 3.55 moles of N2 and 2.50 moles of O2: What is the total pressure for the sample of air described above, if the volume is 29.51 L and the temperature is 300. Kelvin? O 5.06 atm 03.13 atm 01.01 atm 4.25 atm
Question 22 (2.5 points) How many grams of glucose (C6H1206) are in 3.55 moles of glucose?...
Question 22 (2.5 points) How many grams of glucose (C6H1206) are in 3.55 moles of glucose? A) 180. g B) 639 g C) 103 g D) 426 g E) 50.7 g А с ОЕ B D Question 23 (2.5 points) How many grams of MgO are produced when 40.0 grams of O2 react completely with Mg in the following reaction? 2Mg (s) + O2(g) → 2MgO(s) A) 30.4 g B) 50.4 g C) 60.8 g D) 101 g E) 201...
for this question A sample of gas contains 0.1900 mol of N2(g) and 0.3800 mol of...
for this question A sample of gas contains 0.1900 mol of N2(g) and 0.3800 mol of H2(g) and occupies a volume of 20.6 L. The following reaction takes place: N2(g) + 2H2(g) —>NH49) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant L A sample of krypton gas collected at a pressure of 1.40 atm and a temperature of 26.0 °C is found to occupy a volume of 28.8...
Question 22 (3 points) Determine the total pressure of a mixture of 30.0 g of N2,...
Question 22 (3 points) Determine the total pressure of a mixture of 30.0 g of N2, 54.4 g of O2, and 13.3 g of H2 in a 3.00 L container at a temperature of 300.0°C Your Answer: Answer units
Question 7 (1 point) A sample of gaseous neon has a volume of 68.2 Lat STP....
Question 7 (1 point) A sample of gaseous neon has a volume of 68.2 Lat STP. How many moles of neon are in the sample? 0.328 moles 3.04 moles 68.2 moles 1530 moles 4.11 X 1025 moles Question 8 (1 point) The temperature of a gas at 1.00 atm and 8.00°C is increased to 20.0°C resulting in a change of pressure. Which equation would you use to calculate the new pressure? P: V1 = PzV2 OP/V1 = P2/V2 O P₂...
*SHOW YOUR WORK* (Boyle's Law): 1. What is the final volume (in mL) or argon gas...
*SHOW YOUR WORK* (Boyle's Law): 1. What is the final volume (in mL) or argon gas is 50.0 mL at 705 torr is compressed to a pressure of 2.75 atm, at constant temperature? (Lewis Dot Structures): 2. Draw Lewis structures for the following molecules. Include partial charges, AXE designation, (example: AX2 E2), Electron-pair geometry and geometric-molecular shapes. Is it Polar or Non-Polar? CH2Cl2 SO2 3. Which of the following explains why the pressure of a gas increases when the temperature...
I would like the answer for two questions. question 29 and question 46 All of the...
I
would like the answer for two questions. question 29 and question
46
All of the above are correct. Question 46 (2 points) What is the initial pressure of a gas having an initial temperature of 90.5K, an initial volume of 40.3 L, a final pressure of 0.83 atm, a final temperature of 0.54 K and a final volume of 2.7 L O4.0 atm 1.3 atm 1.9 atm 0.074 uestion 47 (2 points) ✓ Saved The density of is 0.900...
Combined Gas Relationship Since the Ideal Gas Law produces a constant (R), it can be used...
Combined Gas Relationship Since the Ideal Gas Law produces a constant (R), it can be used to look at a gas sample in which initial and final conditions have changed. The combined gas relationship is as follows P.V R=P.V2 n, T n2 T2 where P, Vi,and T, and n, are the initial pressure, volume, temperature, and number of moles of gas. The final conditions are represented by P, V2, T2 and n2. If any of the conditions in the initial...
If you have ever hiked or climbed to high altitudes in the mountains, you surely have...
If you have ever hiked or climbed to high altitudes in the mountains, you surely have noticed how short of breath you get. This occurs because the air is thinner, so each breath contains fewer O2 molecules than at sea level. At the top o Mt. Everest, the pressure is only atm Air contains 21.0% O2 and 78.0% N2, and an average human breath is 0.450 L of air. For related problem-solving tips and strategies, you may want to view...
1Q) A nitrogen sample occupies 220. mL at STP. If the same sample were collected over...
1Q) A nitrogen sample occupies 220. mL at STP. If the same sample were collected over water at 25°C and 600. torr, what would be the volume of the gas sample? (Assume that vapor pressure of water at 25°C is 23.8 torr.) Volume =....... mL 2Q) A number of compounds containing the heavier noble gases, and especially xenon, have been prepared. One of these is xenon hexafluoride (XeF6), which can be prepared by heating a mixture of xenon and fluorine...
Question 21 (4 points) Saved A sample of air has 3.55 moles of N2 and 2.50 moles of O2: What is the total pressure for the sample of air described above, if the volume is 29.51 L and the temperature is 300. Kelvin? O 5.06 atm 03.13 atm 01.01 atm 4.25 atm
Question 22 (2.5 points) How many grams of glucose (C6H1206) are in 3.55 moles of glucose? A) 180. g B) 639 g C) 103 g D) 426 g E) 50.7 g А с ОЕ B D Question 23 (2.5 points) How many grams of MgO are produced when 40.0 grams of O2 react completely with Mg in the following reaction? 2Mg (s) + O2(g) → 2MgO(s) A) 30.4 g B) 50.4 g C) 60.8 g D) 101 g E) 201...
for this question A sample of gas contains 0.1900 mol of N2(g) and 0.3800 mol of H2(g) and occupies a volume of 20.6 L. The following reaction takes place: N2(g) + 2H2(g) —>NH49) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant L A sample of krypton gas collected at a pressure of 1.40 atm and a temperature of 26.0 °C is found to occupy a volume of 28.8...
Question 22 (3 points) Determine the total pressure of a mixture of 30.0 g of N2, 54.4 g of O2, and 13.3 g of H2 in a 3.00 L container at a temperature of 300.0°C Your Answer: Answer units
Question 7 (1 point) A sample of gaseous neon has a volume of 68.2 Lat STP. How many moles of neon are in the sample? 0.328 moles 3.04 moles 68.2 moles 1530 moles 4.11 X 1025 moles Question 8 (1 point) The temperature of a gas at 1.00 atm and 8.00°C is increased to 20.0°C resulting in a change of pressure. Which equation would you use to calculate the new pressure? P: V1 = PzV2 OP/V1 = P2/V2 O P₂...
I
would like the answer for two questions. question 29 and question
46
All of the above are correct. Question 46 (2 points) What is the initial pressure of a gas having an initial temperature of 90.5K, an initial volume of 40.3 L, a final pressure of 0.83 atm, a final temperature of 0.54 K and a final volume of 2.7 L O4.0 atm 1.3 atm 1.9 atm 0.074 uestion 47 (2 points) ✓ Saved The density of is 0.900...
Combined Gas Relationship Since the Ideal Gas Law produces a constant (R), it can be used to look at a gas sample in which initial and final conditions have changed. The combined gas relationship is as follows P.V R=P.V2 n, T n2 T2 where P, Vi,and T, and n, are the initial pressure, volume, temperature, and number of moles of gas. The final conditions are represented by P, V2, T2 and n2. If any of the conditions in the initial...
If you have ever hiked or climbed to high altitudes in the mountains, you surely have noticed how short of breath you get. This occurs because the air is thinner, so each breath contains fewer O2 molecules than at sea level. At the top o Mt. Everest, the pressure is only atm Air contains 21.0% O2 and 78.0% N2, and an average human breath is 0.450 L of air. For related problem-solving tips and strategies, you may want to view...
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