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What is the pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide 1.73 g of sulfur dioxide and 3.33 g of argon at 42 degrees Celsius?
To find the total pressure in the vessel, you need to calculate the partial pressures of each gas using the ideal gas law. First, calculate the moles of each gas using the given mass and molar mass of each gas. Then, use the partial pressure formula (P = nRT/V) to find the partial pressure of each gas. Finally, sum up the partial pressures to get the total pressure in the vessel.
How do you get the same amount of oxygen to dissolve in plasma as carbon dioxide you would have to?
To get the same amount of oxygen to dissolve in plasma as carbon dioxide, you would need to increase the partial pressure of oxygen in the gas phase. This increase in pressure would drive more oxygen molecules to dissolve into the plasma to reach equilibrium with the gas phase. The solubility of a gas in a liquid is determined by Henry's Law, which states that the amount of gas dissolved is directly proportional to its partial pressure in the gas phase.
If a vessel under 2.015 ATM pressure conains N2 na d water vapor What is the partial pressure of the water vapor if partial pressure of N2 is 1.908?
To find the partial pressure of water vapor in the vessel, subtract the partial pressure of N2 from the total pressure: Partial pressure of water vapor = Total pressure - Partial pressure of N2 = 2.015 ATM - 1.908 ATM = 0.107 ATM.
How does the partial pressure of Carbon Dioxide in the atmosphere vary with temperature?
The partial pressure of carbon dioxide in the atmosphere generally increases with higher temperatures. Warmer temperatures can enhance the release of carbon dioxide from sources such as the oceans and soil, leading to a higher concentration in the atmosphere. Conversely, colder temperatures can result in lower levels of carbon dioxide.
What is the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide 3 moles of nitrogen and 1 mole of hydrogen and has a total pressure of 1.05 ATM?
The total moles of gas in the container is 9 moles (5 moles CO2 + 3 moles N2 + 1 mole H2). To find the partial pressure of CO2, divide the moles of CO2 by the total moles of gas and multiply by the total pressure: (5 moles CO2 / 9 moles total gas) * 1.05 ATM = 0.5833 ATM. Therefore, the partial pressure of CO2 in the container is 0.5833 ATM.
In deoxygenated blood is the partial pressure of carbon dioxide is greater than the partial pressure of oxygen left?
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The partial pressure of carbon dioxide in venous blood is approximately?
The partial pressure of carbon dioxide in venous blood is around 40 mmHg.
How does one calculate alveolar carbon dioxide partial pressure?
Alveolar carbon dioxide partial pressure can be calculated using the alveolar gas equation: PaCO2 = (Pb-PH2O) * FiCO2 - (PaCO2 / R), where PaCO2 is the alveolar partial pressure of carbon dioxide, Pb is barometric pressure, PH2O is water vapor pressure, FiCO2 is inspired fraction of CO2, and R is the respiratory quotient. This equation helps estimate the partial pressure of CO2 in the alveoli.
A breathing mixture used by deep-sea divers contains helium oxygen and carbon dioxide What is the partial pressure of oxygen at 1 atmosphere if P He- 609.5 mm Hg and PC02 equals 0.5 mm Hg?
To find the partial pressure of oxygen, you can subtract the partial pressures of helium and carbon dioxide from the total pressure of 1 atmosphere (760 mm Hg). Partial pressure of oxygen = Total pressure - Partial pressure of helium - Partial pressure of carbon dioxide = 760 mm Hg - 609.5 mm Hg - 0.5 mm Hg = 150 mm Hg.
What blood gas is value with a pH of 7.34 a partial pressure of oxygen of 80mmHg partial pressure of carbon dioxide of 49mmHg and HCO3 of 24mmHg?
metabolic acidosis
What is PaCO2?
The concentration of Carbon Dioxide in arterial blood. Partial (Pa) Carbon Dioxide (CO2) pressure in ABG.
How is the movement of oxygen different from the movement of carbon dioxide in the body?
because your mind is not working
What is responsible for the partial melting of peridotite beneth the mid-ocean ridges?
An increase in pressure.
What is Normal arterial partial pressure torr?
The normal arterial partial pressure of oxygen (PaO2) is typically between 75-100 mmHg when measured at sea level in a healthy individual. Normal arterial partial pressure of carbon dioxide (PaCO2) is usually between 35-45 mmHg.
Where is the greatest partial pressure of CO2?
The greatest partial pressure of CO2 is typically found in the alveoli of the lungs, where CO2 is exchanged between the bloodstream and the air we breathe. This is the point where oxygen is taken in and carbon dioxide is released.
What is the partial pressure of carbon dioxide in the blood returning to the lungs from the body?
The partial pressure of carbon dioxide in the blood returning to the lungs from the body is around 45 mmHg. This is because carbon dioxide is produced as a waste product of cellular respiration in the body's tissues, and it diffuses into the blood to be transported back to the lungs for exhalation.
What is the pH of carbonic acid?
It depends on the partial pressure of the gaseous carbon dioxide, but its pH value is usually 5.7 .
