Calculate the number of liters occupied at stp. a. 1.7 mol h2. b. 1.8 x10(-2) mol n2. c. 2.5 x10(2) mol o2

Ideal Gas equation will be used assuming all the gases are acting Ideally,

                                                 P V  =  n R T
Solving for V,
                                                 V  =  n R T / P    (1)

Standard Temperature  = 273 K

Standart Pressure  =  1 atm

Gas Constant R  =  0.08206 atm.L.mol⁻¹.K⁻¹

1) For 1.7 mole of H₂;
                                    Putting values in eq.1,

                   V  =  (1.7 mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 273 K) ÷ 1 atm

                   V  =  38.08 L

2) For 1.8 ×10⁻² mole of N₂;
                                    Putting values in eq.1,

                   V  =  (1.8 ×10⁻² mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 273 K) ÷ 1 atm

                   V  =  0.403 L

3) For 2.5 ×10² mole of O₂;
                                    Putting values in eq.1,

                   V  =  (2.5 ×10² mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 273 K) ÷ 1 atm

                   V  =  5600 L

Sorry i dont understand the question can you rephase it?

Sorry i dont understand the question can you rephase it?