Consider the overall reaction for the thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen: Consider the thermal decomposition of phosphine which is a first onder reaction. The half-life of the reaction is 35.0 s at 680C. 4PH3(g)P4(g)+6H2(g) How long (in seconds) would it take for 95% of the phosphine to decompose? BACKGROUND Hint: Use the rate constant you calculated in Question 10. The half-life (t1/2 ) is the time required for the concentration of a reactant to Round your answer to the necrest whole number decrease to talf of itsinitial concentration. The integrated rate laws can be solved for time to give an equation for half-life: Below are the integrated rate lanw equations (first equation) aloosg with their simplified half-life equations (second equation) are: - Zero order [A]t=kt+[A]0tt1=2tA)k - First order ln(A]tt=kt+ln[A]0=t0cos - Second order N41=kt+1451tf=2N41 Consider the thermal decomposition of phosphine which is a first order reaction. The half-life of the reaction is 35.0s at 680C. What is the rate constant ( in s1 ) for this reaction? Round your answer to EOUR places past the decimal