Use the general Gas Law, but be careful to use correct units!
p.V=n.R.T
so
n = [p.V] / [R.T]
in which:
or = 8.314 [Pa.m3.K-1.mol-1] when SI-units are used.
According to the ideal gas law, all gases occupy about 22.4 liters per moleof space at standard temperature and pressure, so 22.4x2.56=57.34 liters.
The pressure is 2,02 atmospheres.
the reaction would shift to favor the side with the most moles of gas
the reaction would shift to favor the side with the most moles of gas. (apex).
the reaction would shift to favor the side with the most moles of gas. (apex).
At standard temperature and pressure, 1 mole of any gas will occupy 22.4 liters. Set up a direct proportion of 22.4 liters/1 mole = 1 liter/x moles and solve for x. You get 0.045 moles.
According to the ideal gas law, all gases occupy about 22.4 liters per moleof space at standard temperature and pressure, so 22.4x2.56=57.34 liters.
The volume you would expect the gas to occupy if the pressure is increased to 40 kPa would be 50 liters.
The answer would depend on the pressure attained by the cooker.
1 mole of sodium carbonate + 2 moles of Hydrochloric acid would produce 1 mole of Carbon Dioxide which would occupy 22.4 liters at standard temperature and pressure
sfaas
The pressure is 2,02 atmospheres.
the reaction would shift to favor the side with the most moles of gas
No. Not at anything like normal pressure.
Using the ideal gas law (using torr instead of atm), we calculate that there would be .046 moles of CO, or 2.7x1022 molecules of carbon monoxide.
the reaction would shift to favor the side with the most moles of gas
8.10 L