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∙ 12y agoGraham's law of effusion.
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∙ 12y agoRoot mean square velocity is the measure of the velocity of gas particles that is used for solving problems. It is the square root of the average velocity-squared of the molecules in a gas. The formula for root mean square velocity is sqrt(3RT/Mm) where Mm is the molar mass of the gas in kg / mole, R is the gas constant, and T is the temperature in kelvin.
The formula is either:Na2CO3 (sodium carbonate) with molar mass 105.9884 g/mol (anhydrous),orNaHCO3 (sodium bicarbonate) with molar mass 84.01 g/mol,butNaCO3 doesn't exist.
Molar mass of all oxygen in compound/Total molar mass of compound * 100 = % oxygen in compound ==================
The answer is simple it's one/1
The pH of a solution is a measure of the molar concentration of hydrogen ions in the solution and as such is a measure of the acidity or basicity of the solution. The letters pH stand for power of hydrogen and numerical value for pH is just the negative of the power of 10 of the molar concentration of H+ ions.
The rate of effusion of gases is inversely proportional to the square root of their molar masses. By comparing the molar masses of the two gases, you can determine which gas effuses faster. The gas with the lower molar mass will effuse more quickly.
Graham's law of effusion states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. In other words, lighter gases effuse or diffuse at a faster rate than heavier gases under the same conditions.
The effusion rate of a gas is inversely proportional to the square root of its molar mass. This means that lighter gases effuse faster than heavier gases. This relationship is described by Graham's law of effusion.
No, lighter gases effuse faster than heavier gases. This is because the rate of effusion is inversely proportional to the square root of the molar mass of the gas. Lighter gases have lower molar masses, which results in faster effusion speeds.
The rate of effusion of nitrogen is slightly lower than that of oxygen due to nitrogen being a slightly heavier molecule than oxygen. This is based on Graham's law, which states that the rate of effusion is inversely proportional to the square root of the molar mass of the gas.
molar mass of the gas. This means that lighter gas molecules effuse at a faster rate than heavier gas molecules at the same temperature.
The ratio of effusion rates is inversely proportional to the square root of the molar masses of the gases. The molar mass of H₂ is about 2 g/mol, and the molar mass of UF₆ is around 352 g/mol. Therefore, the ratio of effusion rates for H₂ to UF₆ is approximately √(352/2) which is about 13.3:1.
Assuming they are at the same temperature, ammonia will effuse most rapidly due to its lower molar mass compared to the other three gases. Effusion rate is inversely proportional to the square root of molar mass.
The variables involved in Graham's law are the molar mass of the gas particles and the rate of diffusion or effusion of the gas. The rate of diffusion or effusion is inversely proportional to the square root of the molar mass of the gas particles.
The rate of effusion of a gas is inversely proportional to the square root of its molar mass. Helium has a molar mass of 4.0 g/mol, while sulfur dioxide has a molar mass of 64 g/mol. Therefore, the rate of effusion of SO2 will be √(4.0/64) = 1/4 times that of helium. In other words, sulfur dioxide will effuse more slowly than helium.
No, oxygen does not effuse 1.07 times faster than nitrogen. The effusion rate of a gas is inversely proportional to the square root of its molar mass, so the effusion rate of oxygen would be √(Molar mass of nitrogen / Molar mass of oxygen) ≈ √(28.02 / 32) ≈ 0.91 times faster than nitrogen.
The slowest rate of effusion will be exhibited by the gas with the highest molar mass. For example, Xenon will diffuse at a slower rate than Helium, and chlorine will diffuse at a slower rate than fluorine.