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Is hydrogen a ideal gas?
Hydrogen is close to an ideal gas under certain conditions, particularly at low pressure and high temperature. However, deviations from ideal behavior can occur at high pressure and low temperature due to intermolecular interactions and molecular size effects.
Why ammonia doesnt behave as an ideal gas?
NH3, as in Ammonia, like all real gases, are not ideal. Ideal gases follow the ideal gas laws, but ammonia does not adhere to a few of them. First of all, the volume of its molecules in a container is not negliggible. Next, NH3 molecules have intermolecular hydrogen bonding, which is a strong intermolecular bond. Thus, the forces of attaction between molecules is not neglible. All real gases have a certain degree of an ideal gas, but no real gas is actually ideal, with H2 being the closest to ideal.
How many liters of ammonia gas can be formed from 13.7 L of hydrogen gas at 93.0 C and a pressure of 40.0kPa?
At a constant temperature and pressure a mole of any gas has the same volume. So all you need to know to answer this question is that there are two atoms of hydrogen in a molecule of hydrogen gas and three atoms of hydrogen in a molecule of ammonia gas. 13.7 L * 2/3 = 9.13 L. You can check this by plugging the values into the ideal gas equation, pV = nRT (look on Wikipedia for "Ideal gas law")
How you Find the number of liters of hydrogen gas in 20 g of hydrogen at STP?
First find moles hydrogen gas. 20 grams H2 (1 mole H2/2.016 grams) = 9.921 moles H2 Now, the ideal gas equation. PV = nRT (1 atm)(volume L) = (9.921 moles H2)(0.08206 L*atm/mol*K)(298.15 K) Volume of hydrogen gas = 243 Liters ----------------------------------------------------
What volume will 454 grams of hydrogen occupy at 1.05 ATM and 25 degrees Celsius?
Using the ideal gas law, you can calculate the volume of hydrogen gas as follows: ( V = \frac{{nRT}}{{P}} ). First, you need to find the moles of hydrogen by dividing the mass by the molar mass of hydrogen. Then, plug in the values for moles, gas constant (R), temperature, and pressure to calculate the volume.
Is hydrogen a ideal gas?
Hydrogen is close to an ideal gas under certain conditions, particularly at low pressure and high temperature. However, deviations from ideal behavior can occur at high pressure and low temperature due to intermolecular interactions and molecular size effects.
How many moles of of hydrogen gas occupy 112L at stp?
Ideal gas equation. PV = nRT ===============
Which gas has properties most similar to an ideal gas N2 O2 He Xe?
The gas that has properties most similar to an ideal gas among the options given is helium (He). Helium is a monatomic gas with low molecular weight and weak intermolecular forces, making it behave more closely to an ideal gas compared to the diatomic gases such as N2 and O2, or heavier gases like Xe.
When is H2 an ideal gas?
Hydrogen gas (H2) behaves most closely to an ideal gas at high temperatures and low pressures. In these conditions, the distances between gas particles are large enough to minimize intermolecular forces, resulting in behavior that closely follows the ideal gas law.
Why ammonia doesnt behave as an ideal gas?
NH3, as in Ammonia, like all real gases, are not ideal. Ideal gases follow the ideal gas laws, but ammonia does not adhere to a few of them. First of all, the volume of its molecules in a container is not negliggible. Next, NH3 molecules have intermolecular hydrogen bonding, which is a strong intermolecular bond. Thus, the forces of attaction between molecules is not neglible. All real gases have a certain degree of an ideal gas, but no real gas is actually ideal, with H2 being the closest to ideal.
What is the total volume of hydrogen gas produced with 5.00 grams of zinc react with HCl?
To calculate the total volume of hydrogen gas produced, you would need to use the ideal gas law equation, PV = nRT. First, find the number of moles of hydrogen gas produced using the stoichiometry of the reaction. Then, use the ideal gas law equation along with the conditions (pressure, volume, and temperature) to find the total volume of hydrogen gas produced.
How determine density of gas on hedrogen?
Hydrogen? You need the conditions, pressure and temperature, of the gas. 1 mole of the gas occupies 22.4 liters at STP. The molar mass of hydrogen is 2.0 g/ mole. So the density at STP is 2.0 / 22.4 = 0.0893 g/liter. At any other pressure and temperature you can use the ideal gas law to find the volume of one mole and then find the density.
What is meant by the term 'ideal gas'?
An ideal gas is a theoretical gas composed of a set of randomly-moving, non-interacting point particles. The ideal gas concept is useful because it obeys the ideal gas law. At normal conditions such as standard temperature and pressure, most real gases behave qualitatively like an ideal gas. Many gases such as air, nitrogen, oxygen, hydrogen, noble gases, and some heavier gases like carbon dioxide can be treated like ideal gases within reasonable tolerances.
Why is the pressure of acetic acid in gas phase lower than predictyed by ideal gas law?
The pressure of acetic acid in the gas phase is lower than predicted by the ideal gas law due to intermolecular interactions such as hydrogen bonding between acetic acid molecules. These interactions cause the gas molecules to be more attracted to each other, resulting in decreased pressure compared to what would be expected for an ideal gas.
How many liters of hydrogen gas at STP can be produced with 645 grams of baking soda?
To find the volume of hydrogen gas produced, we first need to convert the mass of baking soda (645g) to moles. Then, using the balanced chemical equation for the reaction, we can determine the moles of hydrogen gas produced. Finally, using the ideal gas law at STP, we can convert the moles of hydrogen gas to liters.
Hydrogen sulfide occupies 278.2 cm3 at 26oC and standard pressure What is the mass of the hydrogen sulfide?
To find the mass of hydrogen sulfide, we need to use the ideal gas law equation. The molar volume of an ideal gas at STP (standard pressure and temperature) is 22.4 L/mol. First, convert the given volume to liters (0.2782 L), then calculate the number of moles using the ideal gas law. Finally, multiply the number of moles by the molar mass of hydrogen sulfide (34.08 g/mol) to find the mass.
How many liters of ammonia gas can be formed from 13.7 L of hydrogen gas at 93.0 C and a pressure of 40.0kPa?
At a constant temperature and pressure a mole of any gas has the same volume. So all you need to know to answer this question is that there are two atoms of hydrogen in a molecule of hydrogen gas and three atoms of hydrogen in a molecule of ammonia gas. 13.7 L * 2/3 = 9.13 L. You can check this by plugging the values into the ideal gas equation, pV = nRT (look on Wikipedia for "Ideal gas law")
