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If the temperature is increased What happens to the partial pressure of oxygen in a sample of air?
If the temperature is increased, the partial pressure of oxygen in a sample of air will also increase. This is because as the temperature rises, the oxygen molecules in the air will have greater kinetic energy and will exert more pressure.
A sample of dry air contains 210 mL of oxygen 780 mL of nitrogen and 10.0 mL of all other gases What is the pressure in mm of Hg due to the nitrogen if the total pressure was 1000.0 mm?
Dalton says: "The partial pressure of a (non-condensing) gas in the mixture is proportional to its concentration." Since your total pressure is 1000 mmHg and the volumes all total to 1000 mL, you don't even need to take your shoes off to do the math.The nitrogen's volume is 780 ml of the total 1000 ml so its partial pressure is 780 mmHg of the total 1000 mmHg.
A sample of oxygen gas occupies 320.0 mL at 27C and atmospheric pressure What volume does it occupy at 120C and the same pressure?
419 mL
A sample of oxygen gas has a volume of 150 milliliters at 300k if the pressure of the sample is held constant and the temp raised to 600k the new sample will be?
Using the combined gas law (P1V1/T1 = P2V2/T2), we can calculate the new volume of the oxygen gas sample at 600K. Given P1V1/T1 = P2V2/T2, we have P1 = P2 (pressure is constant), V1 = 150 mL, T1 = 300K, and T2 = 600K. Plugging in these values, we get V2 = (P1 * V1 * T2) / (T1) = (1 * 150 * 600) / (300) = 300 mL. So, the new volume of the oxygen gas sample at 600K would be 300 milliliters.
Why you use chilled sample in Reid vapor pressure method?
Chilling the sample in the Reid vapor pressure test helps to reduce the vapor pressure of the volatile components in the sample, making it easier to measure accurately. This allows for more precise determination of the vapor pressure under controlled conditions.
What happens to the partial pressure of oxygen in a sample of air when the temperature increases?
When the temperature of a sample of air increases, the partial pressure of oxygen also increases.
If the temperature is increased What happens to the partial pressure of oxygen in a sample of air?
If the temperature is increased, the partial pressure of oxygen in a sample of air will also increase. This is because as the temperature rises, the oxygen molecules in the air will have greater kinetic energy and will exert more pressure.
What if oxygen is removed from a sample of air as iron rusts what happen to the partial pressure of oxygen in the air?
it decreases
A sample of ascorbic acid contains 1.50 of carbon and 2.00 of oxygen while another sample of ascorbic acid contains 6.35 of c. How many grams of oxygen does it contain?
23
A sample of dry air contains 210 mL of oxygen 780 mL of nitrogen and 10.0 mL of all other gases What is the pressure in mm of Hg due to the nitrogen if the total pressure was 1000.0 mm?
Dalton says: "The partial pressure of a (non-condensing) gas in the mixture is proportional to its concentration." Since your total pressure is 1000 mmHg and the volumes all total to 1000 mL, you don't even need to take your shoes off to do the math.The nitrogen's volume is 780 ml of the total 1000 ml so its partial pressure is 780 mmHg of the total 1000 mmHg.
A sample of nitrogen gas is collected over water at 20 degrees Celsius. The vapor pressure of water at 20 degrees Celsius is 18 mmHg. What is the partial pressure of the nitrogen if the total pressure?
The total pressure is the sum of the partial pressure of nitrogen and the vapor pressure of water. Therefore, the partial pressure of nitrogen is the total pressure minus the vapor pressure of water. Given that the total pressure is not provided in the question, we need more information to calculate the partial pressure of nitrogen.
A sample of nitric acid contains 50 HNO3 molecules How many oxygen atoms are in this sample?
In each nitric acid molecule (HNO3), there is one oxygen atom. So, in a sample containing 50 HNO3 molecules, there would be 50 oxygen atoms.
A sample of oxygen gas occupies 300.0 mL at 27ºC and atmospheric pressure What volume does it occupy at 150ºC and the same pressure?
423mL
A Sample of a compound contains 64 g of copper and 16 g of oxygen what is the ratio of mass to copper of oxygen?
The ratio of mass of copper to oxygen in the sample is 4:1. This is determined by dividing the mass of copper (64 g) by the mass of oxygen (16 g).
Why high pressure oxygen is used in bomb calorimeter?
There are 2 reasons for using high pressure oxygen in bomb calorimeter. The 1st is that we need enough oxygen for a complete combustion in a very small volume. To do that the oxidant pressure must be high. The typical air ratios in a bomb calorimeter are between 4 and 9. The 2nd reason is that we want to measure the high calorific value of a fuel. Thus the water produced from the combustion must be in liquid form. For a certain temperature, the higher the vapor pressure, the higher the liquid water percentage. So, the higher the total pressure (25 atm), the higher the partial vapor pressure. jimmer
A sample of oxygen gas occupies 320.0 mL at 27C and atmospheric pressure What volume does it occupy at 120C and the same pressure?
419 mL
A sample natural gas contains 8.24 moles of methane 0.421 moles of Ethelin 0.116moles of propane if the total pressure of the gases is 1.77atm what are the partial pressures of the gases?
First you need to find the mole ratio of the gases. So take the moles of the gas and divide it by the total moles. After you've done that, you can set that equal to the partial pressure equation, P1 divided by Ptotal. Multiple Ptotal to both sides and you will get the answer
