- #1

herbertpbarreto

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## Homework Statement

The decomposition of phosphine 4PH3(g) + P4(g) + 6H2(g) is first-order with respect to phosphine with a rate constant k = 0.0155 s-l at 953 K. If the decomposition occurs in a constant-volume batch reactor at 953 K, calculate, for 40% conversion of PH3,

(a) the time required, s;

(b) the mole fraction of H2 in the reaction mixture.

## Homework Equations

(

-rA)=-dCa/dT

(-rA)=kCa

Ca= Ca0 (1-Xa)

## The Attempt at a Solution

a) i attempet do apply the equation for spatial time I am batch reactors:

-dCa/dT = kCa

∫-dCa/Ca =∫kdT

-ln(Ca/Ca0) = kT

-ln (Ca0(1-Xa)/Ca0) = kT

-ln (1-Xa) = kT --> -ln (1-0,4) = 0,0155 * T --> -ln(0,6)/0,0155 =T

T = 32,96 s

b) i have no idea

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