0
No, the vapor pressure of CO2 would be higher. Think of it like this, if you compress the molecules in gas enough, they will be close enough together to form a liquid. Both CO2 and water can exist as liquids and gas. At atmospheric pressure (14.7psi) or normal everyday pressure, water is a liquid and CO2 is a gas. This means that 14.7psi is not enough pressure to compress CO2 into the liquid state. Therefore, CO2 has a higher vapor pressure because it requires more pressure to become a liquid.
Looking at it from the other side, if you had extremely high pressure where CO2 and water were both liquids and you started lowering the pressure, CO2 would become a vapor first once you went below a certain high pressure, and water wouldn't become a gas until you went well below atmospheric pressure.
What else can I help you with?
What statements is true about vapor pressure?
The vapor pressure of 1 m sucrose (C12H22O11) is higher than the vapor pressure of 1 m NaCl where the solvent is water Sea water has a lower vapor pressure than distilled water. The vapor pressure of 0.5 m NaNO3 is the same as the vapor pressure of 0.5 m KBr, assuming that the solvent in each case is water The vapor pressure of 0.10 m KCl is the same as the vapor pressure of 0.05 m AlCl3 assuming the solvent in each case is water The vapor pressure of 1 m NaCl is lower than the vapor pressure of 0.5 m KNO3, assuming that the solvent in each case is water The vapor pressure of 0.10 m NaCl is lower than the vapor pressure of 0.05 m MgCl2 assuming the solvent in each case is water.
Why does air containing large amounts of water vapor have lower pressure than air that is dry?
Air with high water vapor content has lower pressure because water vapor molecules are less dense than nitrogen and oxygen molecules found in dry air. This results in fewer gas molecules per unit volume, leading to lower pressure.
Sea water has a lower vapor pressure than distilled water?
Yes, sea water has a lower vapor pressure than distilled water because the presence of dissolved salts in sea water lowers its vapor pressure. This makes it harder for sea water to evaporate compared to distilled water.
What does the vapor pressure of water at 10 C compare with its vapor pressure at 50 C?
The vapor pressure of water at 10°C is lower than its vapor pressure at 50°C. As temperature increases, the vapor pressure of water also increases because more water molecules have enough energy to escape into the gas phase.
Compare the vapor pressure of water at 10 C with its vapor pressure at 50 C?
Vapor pressure of water at 10 0C is less than that at 50 0C because, like gas pressure, as temperature rises, the kinetic energy of particles increases, thus increasing pressure. So the pressure of water vapor at 50 0C has more vapor pressure than at 10 0C.
How does the vapor pressure of water at 10 degrees celsius compare with its vapor pressure at 50 degrees celsius?
The vapor pressure of water at 10 degrees Celsius is lower than at 50 degrees Celsius. As temperature increases, so does the vapor pressure of water because more water molecules have enough energy to escape into the gas phase.
How will the vapor pressure of pure water compare to an aqueous solution of sodium chloride?
The vapor pressure of pure water will be higher than that of an aqueous solution of sodium chloride at the same temperature because the presence of sodium chloride reduces the number of water molecules available to evaporate, lowering the vapor pressure of the solution. In other words, the solute particles in the solution interfere with the evaporation of water molecules, resulting in a lower vapor pressure compared to pure water.
How does the vapor pressure of water at 10 C compare with its vapor pressure at 50 C?
The vapor pressure of water at 50ºC will be greater than that at 10ºC because of the added energy and thus greater movement of the water molecules. If one knows the ∆Hvap at a given temperature, one can calculate the vapor pressure at another temperature. This uses the Clausius-Clapeyron (sp?) equation. It turns out the vapor pressure of water at 10º is 9.2 mm Hg, and that at 50º is 92.5 mm Hg.
Is water vapor more or less dense than dinitrogen under the same conditions of temperature and pressure?
Water vapor is less dense than dinitrogen under the same conditions of temperature and pressure because the molecular weight of water vapor is lower than that of dinitrogen. This difference in molecular weight means that water vapor has fewer molecules present in a given volume compared to dinitrogen, resulting in lower density.
What two characteristics of this layer make it possible to retain this much water vapor on earth?
The two characteristics of the atmosphere that allow it to retain water vapor on Earth are temperature and pressure. Warmer air can hold more water vapor than cooler air, and higher pressure air can hold more water vapor than lower-pressure air. This combination allows for the retention of significant amounts of water vapor in the Earth's atmosphere.
Why does the boiling temperature of water decrease when the water is under reduced pressure such as it is in a higher altitude?
At higher altitudes, there is reduced atmospheric pressure, which leads to a lower boiling point of water. This happens because with lower pressure, it is easier for water molecules to escape into the air as vapor. Therefore, at higher altitudes, water reaches its vapor pressure (boiling point) at a lower temperature than at sea level.
Is the vapor pressure of chloroform less than that of water?
No, the vapor pressure of chloroform is higher than that of Water. The normal boiling point of chloroform is at 61 °C and approx. 39 °C lower than that of water. For calculating vapor pressures of chloroform and water at different pressures you could visit the links below.
