n=PV/RT The answer does not depend on the molecular weight of air (Avogadro's principle).
n=1.2 moles
By decreasing the pressure with the volume kept constant.
decreases
747 mmHg
14kpa
44.98kpa
468ml
By decreasing the pressure with the volume kept constant.
By decreasing the pressure with the volume kept constant.
The amount of any given gas that will dissolve in a liquid at a given temperature is directly proportional to the partial pressure of that gas.
Assuming constant pressure, the answer is:density = 0.789 x 20/15 = 1.052 kg/litre
Henry's law constant for Carbon Dioxide at 20 degrees Celsius is: 1,6*10^3 ATM
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate: the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 L
Not at room temperature. But it is a molecular solid at temperatures below -78 degrees Celsius.
Rigid container holds hydrogen gas at a pressure of 3.0 atmospheres and a temperature of 2 degrees Celsius. The pressure if the temperature is raised to 10 degrees Celsius will be 15 atmospheres based on the law of pressure for gas.
The Celsius scale is in fact based on water, it freezes at 0 degrees and boils at 100 degrees Celsius at 760 mm Hg pressure.
100 degrees Celsius or 212 degrees Fahrenheit
The temperature in Bulgaria is constant! 18 degrees Celsius!