93. 286 grams of N2 gas are placed into a canister with a volume of 7.5...
93. 286 grams of N2 gas are placed into a canister with a volume
of 7.5 L at 150oC. Calculate the pressure exerted by the gas inside
the canister.
a) 17 atm b) 47 atm c) 31 atm d) 1.3 atm e) 0.042 atm
94. Calculate the mass of NaN3 needed for an air bag to produce
100.0 L of N2 gas at 85.0oC and 1.00 atm, using the following
balanced chemical equation. 2 NaN3 (s) → 2 Na (s) + 3 N2 (g)
a) 332 g b) 148 g c) 221 g d) 442 g e) 664 g
95. For which gas do the molecules have the highest average
velocity?
a) He b) Cl2 c) CH4 d) NH3 e) N2
96. Calculate the molar mass for 1.00 gram of gas, which has a
volume of 250. mL at STP.
a) 89.6 g/mol b) 28.0 g/mol c) 14.0 g/mol d) 22.4 g/mol e) 97.9
g/mol
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93. 286 grams of N2 gas are placed into a canister with a volume
of 7.5...
What is the molar mass of a gas that has a density of 2.62 g/L at...
What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0 degree C? 2.69 g/mol 64.0 g/mol 28.0 g/mol 32.0 g/mol 16.0 g/mol What volume is occupied by 1.00 mol of an ideal gas at 1.00 atm and 0.00degreeC? 27.2 L 15.0 L 22.4 L 22.7 L 22.1 L
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a...
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) 2 Na(s) +3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaN3 do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
11. A 0.125 g sample of an unknown gas at 286 K occupies a volume of...
11. A 0.125 g sample of an unknown gas at 286 K occupies a volume of 0.0555 L at a pressure of 0.691 atm. What is the molecular weight of this gas? PV-ART a) 76.5 g/mol m=? P=0.691 to 286k v=0,0555L b) 56.1 g/mol c) 84.2 g/mol d) 79.5 g/mol 23.46916 = 0.016 mol 0.60 (0.0555L) an (0.08206)(2066) 0,0383505 n 23.46916 234691
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a...
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) → 2 Na(s) + 3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaNz do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
QUESTION 1 What will be the pressure of 52.5 grams of oxygen gas in a glass...
QUESTION 1 What will be the pressure of 52.5 grams of oxygen gas in a glass container with a volume of 6 L at 15.4 °C? QUESTION 2 At what temperature in °C does 37.34 g of oxygen gas occupy 18.17 L at 622 mm Hg? QUESTION 3 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g)O2(g)-»2 H20(g) How many grams of water could be produced by the reaction of 5.1 liters of hydrogen with...
Please help with these two questions 1.) Consider the reaction between hydrogen gas and oxygen gas...
Please help with these two questions
1.) Consider the reaction between hydrogen gas and oxygen gas to
form water:
2 H2(g) + O2(g) → 2 H2O(g).
How many grams of water could be produced by the reaction of
4.28 liters of hydrogen with 4.11 liters of oxygen at STP?
2.) Automobile airbags use the decomposition of sodium azide,
NaN3, to provide gas for rapid inflation:
2 NaN3(s) → 2 Na(s) + 3 N2(g).
Using stoichiometry and the ideal gas law,...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation 2 NaN3(s) - 2 Na(s) + 3 N2(9) Using stoichiometry and the ideal gas law, calculate the mass (ing) of NaN3 required to provide 42 L of N2(g) at 28.3 °C and 1.00 atm?
A) Compute the specific heat capacity at constant volume of nitrogen (N2) gas. The molar mass...
A) Compute the specific heat capacity at constant volume of nitrogen (N2) gas. The molar mass of N2 is 28.0 g/mol. the answer is: 741 J/(kg*k) B) You warm 1.55kg of water at a constant volume from 23.0?C to 29.0?C in a kettle. For the same amount of heat, how many kilograms of 23.0?C air would you be able to warm to 29.0?C? Make the simplifying assumption that air is 100% N2. C) What volume would this air occupy at...
Calculate the mass of nitrogen present in a volume of 3000 cm3 if the temperature of...
Calculate the mass of nitrogen present in a volume of 3000 cm3 if the temperature of the gas is 22.0 ∘C and the absolute pressure 2.00×10−13 atm is a partial vacuum easily obtained in laboratories. The molar mass of nitrogen (N2) is 28.0 g/mol . Express your answer in kg
1.What volume of O2 (at 0.855 atm and 26.5 oC) is produced by the decomposition of...
1.What volume of O2 (at 0.855 atm and 26.5 oC) is produced by the decomposition of 6.45 kg of HgO? 2HgO(s) --> 2 Hg(l) + O2(g) 2.Automobile airbags are inflated by the rapid decomposition of sodium azide (NaN3). 2 NaN3(s) --> 2 Na(s) + 3 N2(g) What volume of N2 gas, at 0.861 atm and 26.3 oC, is produced by the complete decomposition of 110 g of sodium azide? 3.What is the root-mean-square (RMS) speed of N2 molecules at 298...
What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0 degree C? 2.69 g/mol 64.0 g/mol 28.0 g/mol 32.0 g/mol 16.0 g/mol What volume is occupied by 1.00 mol of an ideal gas at 1.00 atm and 0.00degreeC? 27.2 L 15.0 L 22.4 L 22.7 L 22.1 L
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) 2 Na(s) +3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaN3 do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
11. A 0.125 g sample of an unknown gas at 286 K occupies a volume of 0.0555 L at a pressure of 0.691 atm. What is the molecular weight of this gas? PV-ART a) 76.5 g/mol m=? P=0.691 to 286k v=0,0555L b) 56.1 g/mol c) 84.2 g/mol d) 79.5 g/mol 23.46916 = 0.016 mol 0.60 (0.0555L) an (0.08206)(2066) 0,0383505 n 23.46916 234691
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) → 2 Na(s) + 3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaNz do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
QUESTION 1 What will be the pressure of 52.5 grams of oxygen gas in a glass container with a volume of 6 L at 15.4 °C? QUESTION 2 At what temperature in °C does 37.34 g of oxygen gas occupy 18.17 L at 622 mm Hg? QUESTION 3 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g)O2(g)-»2 H20(g) How many grams of water could be produced by the reaction of 5.1 liters of hydrogen with...
Please help with these two questions
1.) Consider the reaction between hydrogen gas and oxygen gas to
form water:
2 H2(g) + O2(g) → 2 H2O(g).
How many grams of water could be produced by the reaction of
4.28 liters of hydrogen with 4.11 liters of oxygen at STP?
2.) Automobile airbags use the decomposition of sodium azide,
NaN3, to provide gas for rapid inflation:
2 NaN3(s) → 2 Na(s) + 3 N2(g).
Using stoichiometry and the ideal gas law,...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation 2 NaN3(s) - 2 Na(s) + 3 N2(9) Using stoichiometry and the ideal gas law, calculate the mass (ing) of NaN3 required to provide 42 L of N2(g) at 28.3 °C and 1.00 atm?
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