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3. An Erlenmeyer flask is filled with air at atmospheric pressure (assume we are at sea...
An Erlenmeyer flask is filled with air at atmospheric pressure (assume we are at sea level...
An Erlenmeyer flask is filled with air at atmospheric pressure (assume we are at sea level for atmospheric pressure) room temperature. It is placed in an ice bath. The flask is removed from the ice bath and warmed back to room temperature. Calculate the percent change in the two pressure readings.
The atmospheric pressure varies proportionally from sea level to height, and the air temperature ...
The atmospheric pressure varies proportionally from sea level to height, and the air temperature drops by 6K for every T km increase (a) Draw a cylindrical volume that is height inside the atmosphere, and then calculate the pressure change and expression (dP/dy-pg) depending on the height. (b) obtain the temperature change of the atmosphere accordingto the height y(km) in the place where the sea level (y-0) is at ToK temperature. (c) obtain a barometric equation which allows for the change...
At 30,000 feet above sea level, atmospheric pressure is only 224 torr. That’s why airplane cabins...
At 30,000 feet above sea level, atmospheric pressure is only 224 torr. That’s why airplane cabins are pressurized. There isn’t enough air for you to breathe outside the plane! If we took a balloon filled to 3.86L at room temperature (21°C) and 0.947 atm, what would its volume be at 30,000 feet above sea level (outside the airplane!) if the temperature also reduced to -35.°C?
answer asap please A sealed balloon is filled with air at atmospheric pressure (P = 1.01...
answer asap please
A sealed balloon is filled with air at atmospheric pressure (P = 1.01 X 105 Pa) at 30°C (typical conditions for the surface of the Earth in St. Thomas). You take the (sealed) balloon with you on top of Mountain Top, which has an elevation of about 450m, where the average air pressure is 9.6 x 109 Pa. The temperature at the top is 26°C, a bit cooler. 2.5 pts. - a) How big is the balloon...
3) At sea level, where the atmospheric pressure is 1.00 atm, a typical 12-inch party balloon...
3) At sea level, where the atmospheric pressure is 1.00 atm, a typical 12-inch party balloon occupies 14.8 L at room temperature (23 °C). (13 pts) a) What would the volume of the balloon be at the top of Mount Everest (elevation 5.miles), where the temperature is -28 °C and the pressure is 253.0 torr? Assume that no gas is lost while transporting the balloon. (7 pts) b) How many moles of gas are present in the balloon? (6 pts)
Data: Mass of flask filled with air - 150.9425 g Mass of flask filled with CO2...
Data: Mass of flask filled with air - 150.9425 g Mass of flask filled with CO2 Trial 1 - 150.9775 g Mass of flask filled with CO2 Trial 2 - 150.9805 g Average mass flask filled with CO2 - 150.979 g Temperature of CO2 - 296.15 K Barometer reading - 1.0 atm Density of water at room temp - 0.9978g/mL Density of dry air in flask at room temp - 1.201g/L Calculations: Mass of water in flask - 392.85 mL...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of wat...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of water bath (°C) 100t 99.1 Mass of Erlenmeyer flask, rubber band, foil cover and condensed 0819 gas sample (9) Mass of the condensed gas sample (9) 251.59 Barometric (atmospheric) pressure (mmHg) 128.96 28.93 Volume of the Erlenmeyer flask (mL) 170 170 Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): DATA ANALYSIS (Show your calculations) 1. Determine the...
(6 pts.) 1. The air pressure in the inner tube of a tire on a typical...
(6 pts.) 1. The air pressure in the inner tube of a tire on a typical racing bike is held at a pressure of 115 psi (pounds per square inch). Convert this pressure to atm and mm Hg. (3 pts. each) 2. The atmospheric pressure is 0.975 atm. Determine the pressure of the enclosed gas in each of the cases depicted below. 80 47 mm mm Gas Gas (6 pts.) 3. A 4.00 L flask contains 9.00 g of Ne...
P2) (50 pts.) The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pre...
P2) (50 pts.) The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pressure) is -196°C. Therefore, nitrogen is commonly used in low-temperature scientific studies, since the temperature of liquid nitrogen in a tank open to the atmosphere will remain constant at -196°C until it is depleted. Any heat transfer to the tank will result in the evaporation of some liquid nitrogen, which has a heat of vaporization of 198 kJ/kg and a density of 810 kg/m3...
The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pressure) is -196°C. Therefore, nitroge...
The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pressure) is -196°C. Therefore, nitrogen is commonly used in low-temperature scientific studies since the temperature of liquid nitrogen in a tank open to the atmosphere will remain constant at -196°C until it is depleted. Any heat transfer to the tank will result in the evaporation of some liquid nitrogen, which has a heat of vaporization of 198 kJ/kg and a density of 810 kg/m3 at 1 atm....
An Erlenmeyer flask is filled with air at atmospheric pressure (assume we are at sea level for atmospheric pressure) room temperature. It is placed in an ice bath. The flask is removed from the ice bath and warmed back to room temperature. Calculate the percent change in the two pressure readings.
The atmospheric pressure varies proportionally from sea level to height, and the air temperature drops by 6K for every T km increase (a) Draw a cylindrical volume that is height inside the atmosphere, and then calculate the pressure change and expression (dP/dy-pg) depending on the height. (b) obtain the temperature change of the atmosphere accordingto the height y(km) in the place where the sea level (y-0) is at ToK temperature. (c) obtain a barometric equation which allows for the change...
answer asap please
A sealed balloon is filled with air at atmospheric pressure (P = 1.01 X 105 Pa) at 30°C (typical conditions for the surface of the Earth in St. Thomas). You take the (sealed) balloon with you on top of Mountain Top, which has an elevation of about 450m, where the average air pressure is 9.6 x 109 Pa. The temperature at the top is 26°C, a bit cooler. 2.5 pts. - a) How big is the balloon...
3) At sea level, where the atmospheric pressure is 1.00 atm, a typical 12-inch party balloon occupies 14.8 L at room temperature (23 °C). (13 pts) a) What would the volume of the balloon be at the top of Mount Everest (elevation 5.miles), where the temperature is -28 °C and the pressure is 253.0 torr? Assume that no gas is lost while transporting the balloon. (7 pts) b) How many moles of gas are present in the balloon? (6 pts)
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of water bath (°C) 100t 99.1 Mass of Erlenmeyer flask, rubber band, foil cover and condensed 0819 gas sample (9) Mass of the condensed gas sample (9) 251.59 Barometric (atmospheric) pressure (mmHg) 128.96 28.93 Volume of the Erlenmeyer flask (mL) 170 170 Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): DATA ANALYSIS (Show your calculations) 1. Determine the...
(6 pts.) 1. The air pressure in the inner tube of a tire on a typical racing bike is held at a pressure of 115 psi (pounds per square inch). Convert this pressure to atm and mm Hg. (3 pts. each) 2. The atmospheric pressure is 0.975 atm. Determine the pressure of the enclosed gas in each of the cases depicted below. 80 47 mm mm Gas Gas (6 pts.) 3. A 4.00 L flask contains 9.00 g of Ne...
P2) (50 pts.) The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pressure) is -196°C. Therefore, nitrogen is commonly used in low-temperature scientific studies, since the temperature of liquid nitrogen in a tank open to the atmosphere will remain constant at -196°C until it is depleted. Any heat transfer to the tank will result in the evaporation of some liquid nitrogen, which has a heat of vaporization of 198 kJ/kg and a density of 810 kg/m3...
The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pressure) is -196°C. Therefore, nitrogen is commonly used in low-temperature scientific studies since the temperature of liquid nitrogen in a tank open to the atmosphere will remain constant at -196°C until it is depleted. Any heat transfer to the tank will result in the evaporation of some liquid nitrogen, which has a heat of vaporization of 198 kJ/kg and a density of 810 kg/m3 at 1 atm....
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