The total pressure of a gaseous mixture of 2.8 g N2, 3.2 g O2and 0.5 g H2 is 4.5 atm. Calculate the partial pressure of each gas.A) P 1.00 atm; P :1.00 atm; P 2.5 atmB) P 1.00 atm; P 200 atm; P 3.5 atm©) Prz 2.00 atm; Poz:1.50 atm; Pre: 2.5 atmD) P. 1.00 atm; P. :1.00 atm: P - 3.5 atm

The total pressure of a gaseous mixture of 2.8 g N2, 3.2 g O2and 0.5 g

1.	The total pressure of a gaseous mixture of 2.8 g N2, 3.2 g O2and 0.5 g H2 is 4.5 atm. Calculate the partial pressure of each gas.A) P 1.00 atm; P :1.00 atm; P 2.5 atmB) P 1.00 atm; P 200 atm; P 3.5 atm©) Prz 2.00 atm; Poz:1.50 atm; Pre: 2.5 atmD) P. 1.00 atm; P. :1.00 atm: P - 3.5 atm
Answer» case, the TOTAL number of MOLES will bentotal=0.75+0.30+0.15=1.2 molesThis means that you havePN2=(0.75moles)/(1.2moles)×1.56 atm=0.98 atmPO2=(0.30moles)/(1.2moles)×1.56 atm=0.39 atmPCO2=(0.15moles)/(1.2moles)×1.56 atm=0.20 atmThe values don';t add up to GIVE 1.56 atm because they must be rounded to two sig figs, the number of sig figs you have for the moles of each gas.hope this HELPS you please mark the answer as brainlest please please follow me