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If6 g of sodium azide are completely decomposed by the following reaction in a closed container...
Sulphuric acid decomposes into H2O and SOs n,so, (l)- > H20(g)-S03 (g) if 10.0 g of...
Sulphuric acid decomposes into H2O and SOs n,so, (l)- > H20(g)-S03 (g) if 10.0 g of sulphuric acid is completely decomposed in a closed container with a total volume of 3.00 L and no air at 350 C, what will the total pressure in the container be in atmospheres? Assume the volume of the liquid is negligible. Your answer should have three significant figures. Provide your answer below: atm
10. Sodium azide decomposes rapidly to produce nitrogen gas. 2 NaN (s) 2 Na(s) + 3 N (g) How many gram of sodium az...
10. Sodium azide decomposes rapidly to produce nitrogen gas. 2 NaN (s) 2 Na(s) + 3 N (g) How many gram of sodium azide is required to inflate a 60.0 L airbag for a car to a pressure of 1.50 atm at 32 °C? (R=0.08206 L atm/mol-K) a. 2.40 g b. 67.2 g 156 g d234 g e. 351 g
The sodium azide required for automobile air bags is made by the reaction of sodium metal...
The sodium azide required for automobile air bags is made by the reaction of sodium metal with dinitrogen monoxide in liquid ammonia: You have 62.8 g of sodium, a 35.5-L flask containing N2O gas with a pressure of 2.48 atm at 23 °C, and excess ammonia. What is the theoretical yield (in grams) of NaN3? 3 N2O (g) + 4 Na (s) + NH3 (l) ---> NaN3 (s) + 3 NaOH (s) + 2 N2 (g) Mass = g
Reattempt last question below, or select another question Sodium azide, NaNg, is used in air bags because it quickl...
Reattempt last question below, or select another question Sodium azide, NaNg, is used in air bags because it quickly produces nitrogen gas upon decomposition, What volume, in L, of nitrogen gas should theoretically be produced from the decomposition of 10.5 grams of sodium azide on a hot Phoenix day (112°C) with a barometric pressure of 726 Torr? 2 NaNy(s) 2 Na(s) +3 N2(g) LN2 ( Enter an integer or decimal number [more..] License
< Question 24 of 36 > In the reaction, 2 NaN,(s) — 2 Na(s) + 3N2(g)...
< Question 24 of 36 > In the reaction, 2 NaN,(s) — 2 Na(s) + 3N2(g) what mass of sodium azide, NaNz, would be required to produce 611 L of nitrogen, N2, measured at STP? mass: about us careers privacy policy terms of use contact us help
QUESTION 1 A sample of nitrogen gas is sealed into a 18.6 L container at 715.2...
QUESTION 1 A sample of nitrogen gas is sealed into a 18.6 L container at 715.2 torr and 146.8 °C. How many nitrogen molecules are in the container? (Enter your value in E-notation with three significant figures.] QUESTION 2 A sample of carbon monoxide gas occupies a volume of 200 mL at a pressure of 551.9 torr and a temperature of 633 K. What would its temperature be if the volume were changed to 84 mL at a pressure of...
1. Calculate the density (in g/L) of Freon-12, CF2Cl2, at 27.5°C and 0.949 atm. 2. A mixture of 0.222 g of H2, 1.17 g of N2, and 0.828 g of Ar is stored in a closed container at STP. Find the volume (...
1. Calculate the density (in g/L) of Freon-12, CF2Cl2, at 27.5°C and 0.949 atm. 2. A mixture of 0.222 g of H2, 1.17 g of N2, and 0.828 g of Ar is stored in a closed container at STP. Find the volume (in L) of the container, assuming that the gases exhibit ideal behavior. 3. What volume (in L) of O2 at STP is required to oxidize 9.2 L of NO at STP to NO2? WebAssign will check your answer...
Be sure to answer all parts. Liquid nitrogen trichloride is heated in a 2.50-L closed reaction...
Be sure to answer all parts. Liquid nitrogen trichloride is heated in a 2.50-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 753 mmHg at 82°C. What is the partial pressure of each gas in the container? Pressure of Nz: torr Pressure of Cl2:
You may want to reference (Pages 425-430) Section 10.5 while completing this problem. A 1.5-L, container...
You may want to reference (Pages 425-430) Section 10.5 while completing this problem. A 1.5-L, container of liquid nitrogen is kept in closet measuring 1.1 m by 1.2 m by 20 m ▼ Part A that the container is completely ful, that the temperature is 22.9 C, and that the atmospherk pressure is 12 atm, calculate the percent (by volume) of air that would be displaced if all of the liquid nitrogen evaporated (Liquid nitrogen has a density of 0...
In the formation of smog, nitrogen and oxygen gas react to form nitrogen dioxide: N2(g)+2O2(g)→2NO2(g) Part...
In the formation of smog, nitrogen and oxygen gas react to form nitrogen dioxide: N2(g)+2O2(g)→2NO2(g) Part A How many grams of NO2 will be produced when 2.0 L of nitrogen at 870 mmHg and 29 ∘C are completely reacted? Express your answer using two significant figures. mNO2 m N O 2 = When sensors in a car detect a collision, they cause the reaction of sodium azide, NaN3, which generates nitrogen gas to fill the air bags within 0.03 s....
Sulphuric acid decomposes into H2O and SOs n,so, (l)- > H20(g)-S03 (g) if 10.0 g of sulphuric acid is completely decomposed in a closed container with a total volume of 3.00 L and no air at 350 C, what will the total pressure in the container be in atmospheres? Assume the volume of the liquid is negligible. Your answer should have three significant figures. Provide your answer below: atm
10. Sodium azide decomposes rapidly to produce nitrogen gas. 2 NaN (s) 2 Na(s) + 3 N (g) How many gram of sodium azide is required to inflate a 60.0 L airbag for a car to a pressure of 1.50 atm at 32 °C? (R=0.08206 L atm/mol-K) a. 2.40 g b. 67.2 g 156 g d234 g e. 351 g
Reattempt last question below, or select another question Sodium azide, NaNg, is used in air bags because it quickly produces nitrogen gas upon decomposition, What volume, in L, of nitrogen gas should theoretically be produced from the decomposition of 10.5 grams of sodium azide on a hot Phoenix day (112°C) with a barometric pressure of 726 Torr? 2 NaNy(s) 2 Na(s) +3 N2(g) LN2 ( Enter an integer or decimal number [more..] License
< Question 24 of 36 > In the reaction, 2 NaN,(s) — 2 Na(s) + 3N2(g) what mass of sodium azide, NaNz, would be required to produce 611 L of nitrogen, N2, measured at STP? mass: about us careers privacy policy terms of use contact us help
QUESTION 1 A sample of nitrogen gas is sealed into a 18.6 L container at 715.2 torr and 146.8 °C. How many nitrogen molecules are in the container? (Enter your value in E-notation with three significant figures.] QUESTION 2 A sample of carbon monoxide gas occupies a volume of 200 mL at a pressure of 551.9 torr and a temperature of 633 K. What would its temperature be if the volume were changed to 84 mL at a pressure of...
Be sure to answer all parts. Liquid nitrogen trichloride is heated in a 2.50-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 753 mmHg at 82°C. What is the partial pressure of each gas in the container? Pressure of Nz: torr Pressure of Cl2:
You may want to reference (Pages 425-430) Section 10.5 while completing this problem. A 1.5-L, container of liquid nitrogen is kept in closet measuring 1.1 m by 1.2 m by 20 m ▼ Part A that the container is completely ful, that the temperature is 22.9 C, and that the atmospherk pressure is 12 atm, calculate the percent (by volume) of air that would be displaced if all of the liquid nitrogen evaporated (Liquid nitrogen has a density of 0...
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