Question

Calculate t99.9% / t75% for a first order reaction

Answer 1

Explanation:

T99.9= ln(100/100-99.9)/k= ln(1000)/k

T99.9= ln(100/100-99.9)/k= ln(1000)/k= 2.303*3/k

T99.9= ln(100/100-99.9)/k= ln(1000)/k= 2.303*3/kt75= ln(100/100-75)/k = ln(4)/k= 2.303*log(4)/k

T99.9= ln(100/100-99.9)/k= ln(1000)/k= 2.303*3/kt75= ln(100/100-75)/k = ln(4)/k= 2.303*log(4)/k= 2.303* 2*0.3010/k

T99.9= ln(100/100-99.9)/k= ln(1000)/k= 2.303*3/kt75= ln(100/100-75)/k = ln(4)/k= 2.303*log(4)/k= 2.303* 2*0.3010/kt99/t75= 3/0.6020= 5

T99.9= ln(100/100-99.9)/k= ln(1000)/k= 2.303*3/kt75= ln(100/100-75)/k = ln(4)/k= 2.303*log(4)/k= 2.303* 2*0.3010/kt99/t75= 3/0.6020= 5t99 = 5 * t75