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To accurately answer your question about which gas is released in flask A, I would need more context regarding the specific chemical reaction or process occurring in that flask. Different reactions can produce various gases, such as carbon dioxide (CO2), hydrogen (H2), oxygen (O2), or nitrogen (N2). If you provide details about the substances involved or the reaction taking place, I can give a more precise answer.
What else can I help you with?
Was any gas released in the flask with the boiled yeast mixture?
carbon dioxide
What final volume will the gas occupy after the stopcock is open?
The answer will be the sum of the Flask A and Flask B. The Reason: A gas occupies all the space within a container.
How does a gas change shape when it is poured from a small flask into a large flask?
When a gas is poured from a small flask into a large flask, it expands to fill the larger volume of the new container. Unlike liquids and solids, gases have no fixed shape and can compress or expand to occupy the entirety of their surroundings. As a result, the gas will uniformly distribute itself throughout the larger flask, spreading out to maintain consistent pressure and density.
Was gas released in the flask with boiled yeast mixture?
Yes, gas was likely released in the flask with the boiled yeast mixture due to the fermentation process. Yeast metabolizes sugars, producing carbon dioxide and ethanol as byproducts. If the mixture was not completely killed during boiling, any remaining viable yeast could still ferment available sugars, causing gas to form. However, if the yeast was entirely killed during boiling, no gas would be produced.
When the water level is higher inside than outside the flask is the gas pressure in the flask higher than lower than or the same as the atmospheric pressure?
When the water level is higher inside than outside the flask, the gas pressure in the flask is lower than the atmospheric pressure. This is because the weight of the column of water inside the flask creates an additional pressure on the gas inside, reducing its pressure relative to the atmospheric pressure outside.
Was any gas released in the flask with the boiled yeast mixture?
carbon dioxide
When the water level is higher inside than outside the flask is the gas pressure in the flask higher or lower or the same as the atmospheric pressure?
When the water level is higher inside the flask than outside, the gas pressure in the flask would be lower than the atmospheric pressure. This is because the water exerts a partial vacuum on the gas in the flask, reducing its pressure compared to the external atmospheric pressure.
What final volume will the gas occupy after the stopcock is open?
The answer will be the sum of the Flask A and Flask B. The Reason: A gas occupies all the space within a container.
Why should the flask be covered not stoppered?
Covering the flask instead of stoppering it allows for any gas produced during the reaction to escape, preventing pressure build-up that could lead to the flask exploding. Stoppering the flask could trap the gas and result in a dangerous situation.
Was gas released in the flask with boiled yeast mixture?
Yes, gas was likely released in the flask with the boiled yeast mixture due to the fermentation process. Yeast metabolizes sugars, producing carbon dioxide and ethanol as byproducts. If the mixture was not completely killed during boiling, any remaining viable yeast could still ferment available sugars, causing gas to form. However, if the yeast was entirely killed during boiling, no gas would be produced.
When the water level is higher inside than outside the flask is the gas pressure in the flask higher than lower than or the same as the atmospheric pressure?
When the water level is higher inside than outside the flask, the gas pressure in the flask is lower than the atmospheric pressure. This is because the weight of the column of water inside the flask creates an additional pressure on the gas inside, reducing its pressure relative to the atmospheric pressure outside.
A sample of nitrogen gas is stored in a 500.0ml flask at 108kpa and 10.0c the gas is transferred to a 750.0ml flask at 21.0c what is the pressure of nitrogen in the second flask?
To find the pressure of the nitrogen gas in the second flask, you can use the combined gas law equation: P1V1/T1 = P2V2/T2, where P1, V1, and T1 are the initial pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature. Plug in the given values to find the final pressure of nitrogen in the second flask.
What is the total pressure in the flask?
The total pressure in a flask is the sum of the partial pressures of all the gases present in the flask. It can be calculated using the ideal gas law equation, PV = nRT, where P is the total pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin.
Gas is contained in a 125mL flask The actual volume of the flask is 131.5mL What is the volume of the flask in L?
Volume of the flask = 131.5 mL - 125 mL = 6.5 mL = 0.0065 L
Is the volume occupied by the gas in the flask approxmately the same greater or less than before it was heated?
Assuming the flask is sealed - the volume remains the same but the pressure increases
What is true about the pressure of the gas in the flask?
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Flask A contains 2 liters of ch4 g and flask B contains 2 liters of o2 g each gas sample has the same?
The gas particles in both flask A and B will have the same average kinetic energy at the same temperature. This is because temperature is a measure of the average kinetic energy of the gas particles, and since they are at the same temperature, their average kinetic energies will be equal.
