At 0C and 101,325 kPa: the mass of 186 mL nitrogen is 0,232 686 g.
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.
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.
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.
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.
The density of the sample is about 2.14 g/mL
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.
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.
Density = Mass/Volume = 10 g/100 mL = 0.1 grams per millilitre.
Density = Mass/Volume = 25.0/100 g/mL = 0.25 g/mL
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.
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.
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
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.
Density = Mass/Volume = 50mg/6.4ml = 7.8125 mg/ml or 7.8125 grams per litre.
300K
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.
1100