Problem 1 Four hundred grams of nitrogen gas (molecular weight (MW) = 28 g/mole) are stored in a 10-liter container. Determine the pressure of the gas (in atmospheres) as a function of temperature and volume, using an ideal gas law. Recall that the ideal gas law is PV =nRT, where P = pressure (atm), V = volume (liters), n = number of moles (mass of gas (M)/MW), R = ideal gas constant (0.082054 liter atm/mole K), T = absolute temperature (K = C + 273) Solution must be done using a table, where the columns are organized as follows: Problem #, V (L) , T (C), T (K), R (L atm/mole K) , MW (g/mole), M (g), n (mole), and P (atm). All columns must have titles with corresponding units. Titles must be bold, underlined and centered. Make sure to add borders to the table. a. What pressure corresponds to a temperature of 22C? b. What is the pressure if the temperature is changed to 37C? c. What is the pressure if the original temperature (22C) is restored but the volume of the container is reduced to 7 liters? d. What is the pressure if the original 10-liter container contains 300 grams of oxygen (MW = 32 g/mole) at 18C?