Calculate the heat released when 2.00 L of Cl 2 (g)with a density of 1.88 g/L re

Question

Calculate the heat released when 2.00 L of Cl2 (g)with a density of 1.88 g/L reacts with an excess of sodium metailat 25 degreesC and 1 atm to form sodium chloride. I am having problems with the temp and the 1 atmportion. I know you want to get the mass from the volume anddensity of Cl2 (g), I am just not sure what to do afterthat. Please Help Thank You Calculate the heat released when 2.00 L of Cl2 (g)with a density of 1.88 g/L reacts with an excess of sodium metailat 25 degreesC and 1 atm to form sodium chloride. I am having problems with the temp and the 1 atmportion. I know you want to get the mass from the volume anddensity of Cl2 (g), I am just not sure what to do afterthat. Please Help Thank You

Explanation / Answer

Reaction is 2Na(s) + Cl2 (g) ..................>2NaCl(s) Hrxn = 2mol*H0f (NaCl(s)) -{2mol*H0f (Na(s)) + 1molH0f (Cl2 (g))}             = 2mol * (-411.15kJ/mol) - {2mol * (0kJ/mol) + 1mol *(0kJ/mol)}             = -822.30kJ Hence, 822.30kJ of energy released when one mole ofchlorine reacts with enough sodium so heat released when 0.0530molchorine ( 2.00 L of Cl2 (g) with a density of 1.88g/L)  calculated as below. We know that, mass = volume * density                                 =2.0L*1.88g/L = 3.76g Moles = mass / molar mass            =3.76g / 70.906g/mol = 0.0530 mol heat released = (822.30kJ / 1mol of Cl2 )* 0.0530molCl2   = 43.60kJ

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