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A barometer shows the atmospheric pressure to be 762 mm Hg What is the partial pressure of nitrogen if nitrogen is 78 percent of the air?
To find the partial pressure of nitrogen, multiply the atmospheric pressure by the percentage of nitrogen in the air (0.78). Therefore, the partial pressure of nitrogen would be 0.78 * 762 mm Hg, which equals 594.36 mm Hg.
A box with a volume of 22.4 L contains 1.0 mol nitrogen and 2.0 mol hydrogen at 0à Celsius Which of the following statements is true?
The statement that is true is: The partial pressure of nitrogen is equal to the partial pressure of hydrogen in the box. This is because both nitrogen and hydrogen behave ideally and occupy the same volume, so their partial pressures are directly proportional to their mole quantities in the box.
If atmosphere pressure on a certain day is 749 mm Hg what is the partial pressurre of nitrogen given that nitrogen is about 78 of the atmosphere?
To find the partial pressure of nitrogen, you first need to calculate the total pressure exerted by the atmosphere due to nitrogen. Since nitrogen makes up 78% of the atmosphere, you would multiply the total atmospheric pressure (749 mm Hg) by 0.78 to get the partial pressure of nitrogen, which would be 585.22 mm Hg.
What is the partial pressure of nitrogen in air at 1 atmosphere pressure Assume ideal behavior.?
In dry air, nitrogen constitutes about 78% of the atmosphere by volume. Therefore, at 1 atmosphere pressure, the partial pressure of nitrogen would be 0.78 atm. This is calculated by multiplying the total pressure by the mole fraction of nitrogen in air.
What is the partial pressure of oxygen in a balloon?
The partial pressure of oxygen will vary according to where you look. Atmospheric oxygen partial pressure is approximately 21% of the atmospheric pressure of the location at which you measure (typically around 1 atmosphere at sea level, making the partial pressure of oxygen at seal level 0.21 ATM or 21.3KPa). The value varies geographically and with time, but also varies in different tissues of organisms, since not all oxygen available is absorbed, and complex multicellular organisms will have certain tissues (respiring muscle) that use up oxygen, resulting in a lower partial pressure there.normal oxygen partial185.4 kPa or in another unit:100 mmHg in the arterial blood. The partial pressure on the alveolar site is about 105 mmHg.
A barometer shows the atmospheric pressure to be 762 mm Hg What is the partial pressure of nitrogen if nitrogen is 78 percent of the air?
To find the partial pressure of nitrogen, multiply the atmospheric pressure by the percentage of nitrogen in the air (0.78). Therefore, the partial pressure of nitrogen would be 0.78 * 762 mm Hg, which equals 594.36 mm Hg.
A box with a volume of 22.4 L contains 1.0 mol nitrogen and 2.0 mol hydrogen at 0à Celsius Which of the following statements is true?
The statement that is true is: The partial pressure of nitrogen is equal to the partial pressure of hydrogen in the box. This is because both nitrogen and hydrogen behave ideally and occupy the same volume, so their partial pressures are directly proportional to their mole quantities in the box.
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.
What is the partial pressure of atmospheric nitrogen at sea level?
At sea level, the atmospheric pressure is approximately 101.3 kPa (kilopascals). Since nitrogen makes up about 78% of the Earth's atmosphere, the partial pressure of nitrogen can be calculated by multiplying the total atmospheric pressure by the percentage of nitrogen. This results in a partial pressure of approximately 79.1 kPa for nitrogen at sea level.
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.
What is the partial pressure of nitrogen in air at atmospheric pressure (1atm)?
The partial pressure of nitrogen in air at atmospheric pressure (1 atm) is approximately 0.78 atm. This means that nitrogen makes up about 78% of the total atmospheric pressure at sea level.
If atmosphere pressure on a certain day is 749 mm Hg what is the partial pressurre of nitrogen given that nitrogen is about 78 of the atmosphere?
To find the partial pressure of nitrogen, you first need to calculate the total pressure exerted by the atmosphere due to nitrogen. Since nitrogen makes up 78% of the atmosphere, you would multiply the total atmospheric pressure (749 mm Hg) by 0.78 to get the partial pressure of nitrogen, which would be 585.22 mm Hg.
What is the partial pressure of nitrogen in air at 1 atmosphere pressure Assume ideal behavior.?
In dry air, nitrogen constitutes about 78% of the atmosphere by volume. Therefore, at 1 atmosphere pressure, the partial pressure of nitrogen would be 0.78 atm. This is calculated by multiplying the total pressure by the mole fraction of nitrogen in air.
. A mixture of oxygen hydrogen and nitrogen gases exerts a total pressure of 282 kPa. If the partial pressures of oxygen and hydrogen are 110 kPa and 106 kPa respectively what is the partial pressure?
Total pressure = ppO2 + ppH2 + ppN2ppN2 = Total pressure - (ppO2 + ppH2)ppN2 = 282 kPa - (110+106 kPa) = 282kPa - 216kPappN2 = 66 kPa = partial pressure of nitrogen
A mixture of gases with a pressure of 800.0 mm Hg contains 60 percent nitrogen and 40 percent oxygen by volume What is the partial pressure of oxygen in this mixture?
The partial pressure of oxygen in the mixture can be calculated using Dalton's Law of partial pressures. First, convert the percentages to decimal form (60% = 0.60, 40% = 0.40). Then, multiply the total pressure of 800.0 mm Hg by the volume percentage of oxygen (0.40) to find the partial pressure of oxygen in the mixture. This gives a partial pressure of oxygen of 320.0 mm Hg.
What is the partial pressure of oxygen in blood gas a mixture of N2 O2 and CO2 if the partial pr. of Nitrogen 630 mm of Hg and partial pressure of CO2 is 39 mm of Hg?
To find the partial pressure of oxygen, we need to subtract the partial pressures of nitrogen and CO2 from the total pressure of the mixture, which is typically around 760 mmHg at sea level. Therefore, the partial pressure of oxygen would be 760 - 630 - 39 = 91 mmHg.
Why air dissolved in water contains higher proportion of oxygen?
Air contains about 21% oxygen and 78% nitrogen, while water can only dissolve a limited amount of gas. Therefore, the oxygen in air dissolves in water at a higher proportion than nitrogen. This is due to the partial pressure of oxygen being higher in air compared to nitrogen.
