A decomposition reaction of ethylene creates two H_2 molecules for every C_2H_4

Question

A decomposition reaction of ethylene creates two H_2 molecules for every C_2H_4 molecule, along with elemental carbon - black dust. What can complete decomposition of ethylene in a pipeline do to the pressure in that pipeline? The ideal gas law relates all four of the variables discussed so far. It is simple to remember and from it you can derive all of the other relationships. The formula is: pV = nRT Where R = Universal Gas Constant whose values is based on units used for all of the other variables R = 10.73 ft^3 psia/(R lbmole) Boyles Law says if n & T constant, PV = constant. Charles's Law says if n & P constant, V/T = constant Other relationships include if n & V constant, P/T = constant if p & V constant, nT = constant Using the ideal gas law you can figure out any of these relationships and more. pV = nRT p_2V_2/p_1V_1 = n_2RT_2/n_1RT_1 Cancel anything that is constant & solve the equation for what you want to know. Then you can compare any changes p_2V_2/p_1V_1 = n_2RT_2/n_1RT_1 p_2V_2/p_1V_1 = T_2/T_1 p_2 = T_2p_1V_1/T_1V_2

Explanation / Answer

Using the equation:

P1*V1/T1 = P2*V2/T2

Putting values we get:

(150*500)/480 = (P2*200)/600

Solving we get:

P2 = 468.75 psi

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