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How long will it take 10.0ml of nitrogen gas to enfuse through a porius barrier if it has been observed that 92.1 minutes are required for 10.0mL of Cl2 gas to enfuse through the same barrier?
The rate of gas diffusion through a porous barrier is inversely proportional to the square root of its molar mass (that is, a gas four times as heavy diffuses half as fast). The rest is simple arithmetic.
A 110.0 mL sample of nitrogen at 820 torr was compressed to a volume of 83.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
Using Boyle's law (P1V1 = P2V2), the initial pressure is 820 torr, the initial volume is 110.0 mL, and the final volume is 83.0 mL. Solving for P2, we get P2 = (P1V1) / V2 = (820 torr * 110.0 mL) / 83.0 mL = 1088.55 torr. Therefore, the pressure of the trapped nitrogen in the syringe is 1088.55 torr.
A 125.0 mL sample of nitrogen at 790 torr was compressed to a volume of 75.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
Using Boyle's Law (P1V1 = P2V2), we can find the final pressure with the initial pressure (P1 = 790 torr), initial volume (V1 = 125.0 mL), and final volume (V2 = 75.0 mL). Plugging in the values: (790 torr)(125.0 mL) = P2(75.0 mL). Solving for P2 gives a pressure of 1327 torr for the trapped nitrogen.
What is the mass of 63.0 mL of ethanol?
Assuming the density of ethanol is 0.789 g/mL at room temperature, the mass of 63.0 mL of ethanol would be 49.707 grams.
What is the density of a sample that has mass of 77.0 g and a volume of 36 mL?
The density of the sample is about 2.14 g/mL
What would be the mass in grams of 186 mL of nitrogen gas?
To find the mass of nitrogen gas, you need to know the density of nitrogen gas at the given conditions (typically at STP - standard temperature and pressure). The density of nitrogen at STP is about 1.25 g/L. You can use this value to calculate the mass by multiplying the density by the volume given in milliliters.
What volume of hydrogen gas reacts with 12.0 ml of nitrogen gas?
To determine the volume of hydrogen gas that reacts with 12.0 ml of nitrogen gas, you first need to balance the chemical equation for the reaction. From the balanced equation, use the stoichiometry to determine the volume of hydrogen gas that corresponds to the given volume of nitrogen gas.
What is the density of carbon gas if it has mass of 10 grams and occupies a volume of 100 mL?
Density = Mass/Volume = 10 g/100 mL = 0.1 grams per millilitre.
What is the density of carbon dioxide gas if 25.0 g occupies a volume of 100 mL?
Density = Mass/Volume = 25.0/100 g/mL = 0.25 g/mL
How long will it take 10.0ml of nitrogen gas to enfuse through a porius barrier if it has been observed that 92.1 minutes are required for 10.0mL of Cl2 gas to enfuse through the same barrier?
The rate of gas diffusion through a porous barrier is inversely proportional to the square root of its molar mass (that is, a gas four times as heavy diffuses half as fast). The rest is simple arithmetic.
What is the density of CO gas if G occupies a volume of ml?
To calculate the density of carbon monoxide (CO) gas, you need to know its molar mass, which is approximately 28.01 g/mol. Density (ρ) can be calculated using the formula ρ = mass/volume. If you have the volume of CO gas in milliliters (ml), you can convert it to liters (1 ml = 0.001 L) and then use the ideal gas law or the molar volume at standard temperature and pressure (STP) to find the mass. Once you have the mass, divide it by the volume in liters to find the density in g/L.
Density of nitrogen gas?
For a 1 mole sample of nitrogen, the density is 0.0022g/mL. P = 2 atm n = 1 mole T = 310K R = 0.0821 V = nRT/P = 12.73L = 12,730 mL Nitrogen = 28.02 g (Mass of one mole of Nitrogen gas i.e. N2) [2 x 14.01] d = 28.02g/12,730mL = 0.0022g/mL
A 100 ml sample of nitrogen at 810 torr was compressed to a volume of 72 mL in a syringe What was the pressure of trapped nitrogen in torr?
To find the final pressure of the nitrogen, we can use Boyle's Law which states that the pressure and volume of a gas are inversely proportional when temperature is constant. Therefore, 100 mL * 810 torr = 72 mL * final pressure. Solving for final pressure, we get: final pressure = (100 mL * 810 torr) / 72 mL = 1125 torr. So, the pressure of the trapped nitrogen in the syringe is 1125 torr.
What is the density of 50.0mg of a gas which occupies a volume of 6.4 ml?
Density = Mass/Volume = 50mg/6.4ml = 7.8125 mg/ml or 7.8125 grams per litre.
Calculate the temperature of a 969 mL sample of CH4 gas at 104 kPa with a mass of 0.647 g?
300K
What is the mass of 100 mL?
The mass of 100 mL of a substance depends on its density. You would need to know the density of the substance to calculate the mass. Multiplying the volume (100 mL) by the density (in g/mL) will give you the mass in grams.
A 100.0 mL sample of nitrogen at 810 torr was compressed to a volume of 72.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1100
