The volume that the gas sample will occupy at the same temperature and 475 mmHg is 4448 mL. In significant figures, the answer would be 4400 mL
To find this, you can use the Combined Gas Law, (P1V1)/T1=(P2V2)/T2. First, you need to convert your temperature from degrees Celsius to Kelvin. You can do this by adding 273 to 25, which gives you 298 K. Then you can plug in the given values for volume, pressure, and temperature.
The equation should look like this:
(760 mmHg * 2.78 x 103 ml) / 298 K = (475 mmHg * V2) / 298 K
Then you can solve for V2 to find the unknown volume.
1.27*10^3 mL
18.0L
Pv/t = pv/t
2800 ml
Chlorine gas occupies a volume of 25 mL at 300K What volume it occupy at 600k
419 mL
129
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
The volume is 0,046 L.
305 k
280 ml
Chlorine gas occupies a volume of 25 mL at 300K What volume it occupy at 600k
423mL
A sample of gas occupies 1.55L at STP. What will the volume be if the pressure is increased to 50 atm while the temperature remains constant?
419 mL
More pressure means less volume. Calculate the ratio of pressure, then divide the 4.2 liters by that ratio.This assumes: * That the temperature doesn't change. * That the gas behaves like an ideal gas.
129
Volume is a measure of how much space a sample of matter occupies. the SI unit of volume is m3 .
A sample of Ar gas occupies a volume of 1.2 L at 125Β°C and a pressure of 1.0 atm. Determine the temperature, in degrees Celsius, at which the volume of the gas would be 1.0 L at the same pressure.
Volume = how much space an object occupies, that nothing else can occupy at the same time.
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.