You have a closed container filled with 1L of pure air at STP. Assume that this air is made of only nitrogen (79%) and oxygen (21%). What are the partial pressures of nitrogen and oxygen in the box?Hint: X_N = P_N/PTotal= N_N/N_Total

Question

Quizplus · Accepted Answer

X_N=mole fraction of nitrogen N_N=moles of nitrogen N_Total=moles total X₀=mole fraction of oxygen N_o=moles of oxygen Since 79% of the air is nitrogren, the mole fraction (x_N) is .79. (X_N=N_N/NTotal). Likewise, the mole fraction for oxygen is .21. This is calculated by realizing that 79% of the air is nitrogen, therefore 79% of the molecules (or moles) are nitrogen. So, you don't need to know NN or NTotal to calculate this. Partial pressure equations are as follows: XN = P_N/P_Total= N_N/NTotal .79 = P_N/P_Total .79*P_Totall = P_N .79 * 1.0 atm = PN = .79 atm P₀= P_Total- P_N= 1.0 atm - .79 atm = .21 atm

You Have a Closed Container Filled with 1L of Pure