A) Find the gas speed of ethane at 200.0 degrees Celsius. b) What is the rate of effusion of ethane (C2H6) compared to hexane (C6H14) gas at the same temperature?

a. 627.1 m/s

b.  the rate of effusion of ethane = 1.7 faster than hexane

Given

T = 200 + 273 = 473 K

Required

a. the gas speed

b. The rate of effusion comparison

Solution

a.

Average velocities of gases can be expressed as root-mean-square averages. (V rms)  

R = gas constant, T = temperature, Mm = molar mass of the gas particles  

From the question  

R = 8,314 J / mol K  

T = temperature  

Mm = molar mass, kg / mol  

Molar mass of Ethane = 30 g/mol = 0.03 kg/mol

b. the effusion rates of two gases = the square root of the inverse of their molar masses:  

M₁ = molar mass ethane =30

M₂ =  molar mass hexane = 86

the rate of effusion of ethane = 1.7 faster than hexane

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

the product of the pressure and volume is also constant