My dog gets more action than you do.
Gas molecules are spread out. When they are placed under pressure they condense into a liquid.
If the gas is ideal, or nearly so, it must be at or nearly at standard temperature and pressure.
The solubility of gas increases as the temperature decreases.
That is correct
A mole of gas is equal to 6.02 x 1023 gas molecules.
Gas molecules are spread out. When they are placed under pressure they condense into a liquid.
A mole of ideal gas at STP takes up 22.4 L.
If you compress a gas the temperature increases
The pressure of a gas increases with an increase in temperature.
The pressure of a gas increases with an increase in temperature.
This is the molar volume of an ideal gas at a given temperature and pressure.
The volume occupied by 1 mole of diatomic gas particle at NTP ( Normal Temperature & Pressure) is 11.2 L
The temperature decreases
If the gas is ideal, or nearly so, it must be at or nearly at standard temperature and pressure.
The solubility of gas increases as the temperature decreases.
Hydrogen? You need the conditions, pressure and temperature, of the gas. 1 mole of the gas occupies 22.4 liters at STP. The molar mass of hydrogen is 2.0 g/ mole. So the density at STP is 2.0 / 22.4 = 0.0893 g/liter. At any other pressure and temperature you can use the ideal gas law to find the volume of one mole and then find the density.
Yes - as long as the pressure and temperature are constant.