What is the pressure in a 5.00 L tank with 9.40 moles of oxygen at 39.3 °C?
What is the pressure in a 5.00 L tank with 9.40 moles of oxygen at 39.3 °C?
A balloon at 30.0°C has a volume of 222 mL. If the temperature is increased to 58.1°C and the pressure remains constant, what will the new volume be, in ml?
Consider a 5.00-L tank containing 375 g of Ar at a temperature
of 25 °C.
(a) Calculate the pressure in the tank using both the ideal gas law
and the van der Waals equation.
(b) Which correction term, a(n/V)2 or bn, has the great- est
influence on the pressure of this syste
A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm
pressure. What is the final pressure in the flask if an additional
2.00 g of N2 gas is added to the flask and the flask cooled to
-55°C?
a.) 0.987 atm
b.) 1.35 atm
c.) 1.84 atm
d.) 0.255 atm
If 65.0 L of oxygen at 19.0 ∘C and an absolute pressure of 2.35
atm are compressed to 49.6 L and at the same time the temperature
is raised to 58.5 ∘C, what will the new pressure be?
2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid
5.00-L container and they react according to the equation ? ?
CO2(g) + H2(g) ? CO(g) + H2O(g) ? ? K = 2.50 What will be the
concentration of carbon monoxide when equilibrium is reached?
What is the mass of oxygen dissolved in a 7.0L fish
tank when pressure of air is 0.98atm and the mole fraction of
oxygen in air is 0.22. T=25 C degrees, Henry's constant KH for O2
is 1.3 x 10^-3 M/atm at 25 C degrees.
A) 62.9 mg
B) 123.6 mg
C) 48.9 mg
D) 285.4 mg
4.00 moles of HI are placed in an evacuated 5.00 L flask and
then heated to 800 K. The system is allowed to reach equilibrium.
What will be the equilibrium concentration of each species
The concentration of oxygen inside a 5000 L tank at 1 atm is to
reduced by pressure purging prior to charging a fuel into the tank.
The tank is charged with nitrogen up to a high pressure and then
vented down to atmospheric pressure. If the process is repeated,
the concentation of the oxygen will decrease. It is possible to do
this many times in order to ultimately reach desired concentration.
You can assume that a fully charge tank contains...
1) What is the pressure in a 18.2-L cylinder filled with 27.0g
of oxygen gas at a temperature of 329K ?
2) A gas mixture with a total pressure of 765mmHg contains each
of the following gases at the indicated partial pressures: CO2,
129mmHg ; Ar, 208mmHg ; and O2, 191mmHg . The mixture also contains
helium gas.
What mass of helium gas is present in a 12.4-L sample of this
mixture at 276K ?
Calculate the mass of oxygen gas (O2) dissolved in a
5.00 L bucket of water exposed to a pressure of 1.13 atm of air.
Assume the mole fraction of oxygen in air to be 0.210 and the
Henry's law constant for air in water at this temperature to be
1.30 × 10-3 M/atm.
A 5.00 L N2 gas sample at a pressure of 1.20 atm and
temperature of 15.8ºC has a mass of 7.08 g. What is the mass of a
10.0 L H2 gas sample at the same temperature and
pressure as the N2 gas sample?
(a) How many moles of N2 gas are in the sample?
(b) How many moles of H2 gas are in the sample?
(c) At a given temperature and pressure, 5.00 L of N2 are
reacted with...