The reaction has a half-life of 2.40 × 10 seconds when the initial ammonia conce

Question

The reaction has a half-life of 2.40 × 10 seconds when the initial ammonia concentration is 2.00 M. How long does it take for the concentration of ammonia to decrease from 2.00 M to 1.16 M?
t=____ seconds

Question #: 7 The zero-order decomposition of ammonia on a hot tungsten surface proceeds according to 2 NH3(g) N2(g) + 3 H2(g). The reaction has a half-life of 2.40 x 10 seconds when the initial ammonia concentration is 2.00 M. How long does it take for the concentration of ammonia to decrease from 2.oo M to 1.16 M? t= -seconds Report your answer with two significant figures. Do NOT include units in your answer. Use the format 2.2E2 or 2.2E-2 for numbers in scientific notation.

Explanation / Answer

t1/2   = [A0]/2K

K     = [A0]/2 t1/2

     = 2/2*2.4*10^3    = 0.00042M/sec

[A0] -[A] = kt

2-1.16    = 0.00042 *t

0.84        = 0.00042*t

t             = 0.84/0.00042   = 2000seconds >>>>answer

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