Did the calculation wrong. Now I've got
((.71 mol)(8.3145 J/(mol*kelvin))(-273.15 degrees kelvin)) / (2.0*10^4 cm^3) = -0.795699496 atm
Not the right answer for pressure. But at least the proper units.
Err, I put the wrong units and gas constant. Here:
((.71 mol)(8.3145 J/mol K)(-273.15 degrees K)) / (2.0*10^4 cm^3) = P = -80624251.5 kg K / s2
That's not right either. Sigh.
P = nRT / V
Molar mass of CO is 28.010 g mol^-1.
Therefore number of moles in 20 g is 20 g/28.010 g mol^-1 = 0.71 mol.
P = ((.71)(8.314472e15)(-273.15)) / (2.0*10^4 cm^3)
P = -8.062398*10^19 m^3
Is this correct? What do I do now?
The problem:
20 g of dry ice (solid CO2) is placed in a 2.0*10^4 cm^3 container, then all the air is quickly pumped out and the container sealed. The container is warmed to 0 deg C, a temperature at which CO2 is a gas.
a) What is the gas pressure? Give your answer in atm. The gas then undergoes...
2050 is the specific heat capacity of ice, although I'm not sure where I got that number... It seems every site I go to has a different value. Wikipedia is saying 2110 So I'll see if that makes a difference.
It gives me 17.6, which is still wrong. Any other suggestions?
The problem:
On a hot summer day, you decide to make some iced tea. First, you brew 1.50 L of hot tea and leave it to steep until it has reached a temperature of T_tea = 75.0 C. You then add 0.975 kg of ice taken from the freezer at a temperature of T_ice = 0 C. By the time the mix reaches...