If the gas in question was air (I assume gas does not mean gasoline in this case) there would be 1.225g/dm3 at sea level with a pressure of 1013.25 millibars and a temperature of 150C. The container in this case is 1L which is equal to 1dm3 in volume and 1.5g of air will give the container a pressure of 1013.25x1.5/1.225 The result is 1240.71mb. Claudiosanto
800 K
The pressure is 20,68 at.
The pressure is never low enough, nor the temperature high enough to get a perfect match; but at room temp it comes pretty close. This is the answer: 750 K and 20 kPa (I AM THE WISEONE!!)
10 ppm mole multiply by molecular weight of water then divided by sample density
At 1 ATM pressure and 10°F and 10°C krypton is a gas.
17 l
The volume ofhydrogen is 64,84 L.
800 K
The pressure is 20,68 at.
10.13kPa is 0.1 ATM
one mole of all substances contains 6.022 x 10^23 atoms =number of atoms in 22400 cm^3 of any gas at STP
10 inches of water column equals to how much gas pressure?
10 milligrams
10 cubic inches
The pressure is never low enough, nor the temperature high enough to get a perfect match; but at room temp it comes pretty close. This is the answer: 750 K and 20 kPa (I AM THE WISEONE!!)
B. 10 Cubic inches The formula is: po - original gas pressure vo - original volume pf - final gas pressure vf - final volume Po*Vo = Pf*Vf or 5psi x 20 in3 = 10psi x Vf
10 sample of iterrogative