Question

1) You place a 50mL of 0.50M NaOh and 25mL of 0.50M HCl in a coffee cup calorimeter. What is the final temperature of the calorimeter if the initial temperature of the solution is 15.8 degree celsius. ( The change in enthalpy for the reaction is -55.4 kJ/mole H2O) (assume the solution has specific heat and density as water, s=4.184 J/g oC, density=1.00 g/L)

2) It took 3.20 min for 1.00 L N2 to effuse through a porous barrier. How long will it take for 1.00L of Cl2 to effuse under the same condition?

Answer #1

**1) no of mole of HCl reacted = 25*0.5 = 12.5 mmole =
0.125 mole**

**no of mole of NaOH = 50*0.5 = 25 mmole = 0.25
mole**

**amount of heat released(q) = DHrxn*n = -55.4*0.125 =
-6.925 kj**

**amount of heat released(q) = m*s*DT**

**mass of solution = d*v = 1*(50+25) = 75 g**

** 6.925*10^3 = 75*4.184*(x-15.8)**

**x = final temperature = 37.9 c**

**2) r1/r2 = sqrt(M2/M1)**

**rate of diffusion of N2(r1) = 1/3.2 = 0.3125
l/min**

**M1 = 28 g/mol**

**r2 = rate of diffusion of Cl2 = ?**

**M2 = 71 g/mol**

**0.3125/r2 = sqrt(71/28)**

**r2 = rate of diffusion of Cl2 = 0.196 l/min**

**time required for cl2 = amount / rate = 1/0.196 = 5.1
min**

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