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When a gas occupies a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
The volume is 0,046 L.
What volume will 500 mL of gas at 20 c and a pressure of 420 mm Hg occupy if the temperature is reduced to 80 c and the pressure increased to 650 mm Hg?
To solve, use the combined gas law: (P1V1/T1) = (P2V2/T2). Plug in the initial conditions (P1 = 420 mm Hg, V1 = 500 mL, T1 = 20°C), and the final conditions (P2 = 650 mm Hg, T2 = 80°C) to find V2, the final volume. Remember to convert temperatures to Kelvin by adding 273 to the Celsius temperature.
What is the atomic mass of hg?
The atomic mass of mercury (Hg) is 200.59 grams per mole.
What is the mass of mercury Hg?
The atomic mass of mercury (Hg) is approximately 200.59 grams per mole.
What does 500 mm Hg equals?
500 mmHg or 500 torr is a gas pressure approximately 66% of the standard sea level air pressure of 760 torr ... it is the air pressure one would find at an altitude of approximately 3km or 10000 feet ... at sea level, 500 torr would be considered a partial vacuum of 0.66 atm.
When a gas occupies a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
The volume is 0,046 L.
A gas occupies a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
0.05 L
How many milliliters are in 500grams?
1 gram = 1 mL so;500 g = 500 mL34
At 1250 mm Hg and 75 degrees Celsius the volume of a sample of ammonia gas is 6.28 L What volume would the ammonia occupy at STP?
Using the combined gas law, we can relate the initial and final conditions of the gas: P1V1/T1 = P2V2/T2. At STP (Standard Temperature and Pressure), the conditions are 1 atm and 0 degrees Celsius. Convert 1250 mm Hg to atm and 75 degrees Celsius to Kelvin. With this information, you can then calculate the final volume of the ammonia gas at STP.
What volume will 500 mL of gas at 20 c and a pressure of 420 mm Hg occupy if the temperature is reduced to 80 c and the pressure increased to 650 mm Hg?
To solve, use the combined gas law: (P1V1/T1) = (P2V2/T2). Plug in the initial conditions (P1 = 420 mm Hg, V1 = 500 mL, T1 = 20°C), and the final conditions (P2 = 650 mm Hg, T2 = 80°C) to find V2, the final volume. Remember to convert temperatures to Kelvin by adding 273 to the Celsius temperature.
If 7.56 L of a gas are collected at a pressure of 745 mm Hg then what volume will this gas occupy at standard atmospheric pressure if the temperature remains the same?
To find the volume at standard pressure, we can use the combined gas law equation, which states that (P1 x V1) / T1 = (P2 x V2) / T2. Assuming standard pressure is 760 mm Hg, we have: (745 mm Hg x 7.56 L) / T = (760 mm Hg x V2) / T. Solving for V2, we get V2 = (745 x 7.56 x T) / 760. Since the temperature is constant, the volume at standard pressure will be 745 x 7.56 = 5644.2 L.
40 liters of gas were collected over water when the barometer read 622.0 mm Hg and temp was 20C what volume wuould dry gas occupy at standard conditions?
To find the volume of the dry gas at standard conditions (0°C and 1 atm), we need to correct for the water vapor using the vapor pressure of water at 20°C. The vapor pressure of water at 20°C is 17.5 mm Hg. Therefore, the pressure of the dry gas is 622.0 mm Hg (total pressure) - 17.5 mm Hg (water vapor pressure) = 604.5 mm Hg. Using the ideal gas law, we can calculate the volume of the dry gas at standard conditions.
How many 50 hg in dg?
500
What is the atomic mass of hg?
The atomic mass of mercury (Hg) is 200.59 grams per mole.
A 500 ml sample of gas at 760 mm Hg is compressed to 100 ml what is the new pressure?
To find the new pressure after the compression, you can use Boyle's Law, which states that pressure and volume are inversely related at constant temperature. Using the formula P1V1 = P2V2, where P1 = 760 mm Hg, V1 = 500 ml, V2 = 100 ml, you can calculate the new pressure (P2) by rearranging the formula as follows: P2 = P1V1 / V2 = (760 mm Hg * 500 ml) / 100 ml. Substituting these values gives you the new pressure after compression.
What is the mass of mercury Hg?
The atomic mass of mercury (Hg) is approximately 200.59 grams per mole.
How can 1mole of hydrogen gas occupy 22.4ltrs of volume when you know that a gas occupies all the space available to it?
At standard temperature and pressure. This means that, more or less, there are 6.022 X 10^23 diatomic molecules of H2 in that much volume. ( the volume not being under more than standard pressure; 760mm/Hg ) In twice the volume about twice the molecules under STP.
