Chemistry, 06.12.2019 05:31 haitiindianari
Consider the reaction 4 ph3(g) → p4(g) + 6 h2(g). if, in a certain experiment, over a specific time period, 0.0049 mole of ph3 is consumed in a 2.4-l container during each second of the reaction, what are the rates of production of p4 and h2 in this experiment?
Answers: 1
![R=-\frac{1}{4}\frac{d[PH_3]}{dt}=\frac{1}{1}\frac{d[P_4]}{dt}=\frac{1}{6}\frac{d[H_2]}{dt}](/tpl/images/0405/9326/1b2ce.png)
![-\frac{d[PH_3]}{dt}](/tpl/images/0405/9326/0026c.png)
![\frac{[PH_3]}{1 s}](/tpl/images/0405/9326/00de6.png)
![-\frac{d[PH_3]}{dt}=0.002042 M/s](/tpl/images/0405/9326/a6182.png)
![R = -\frac{1}{4}\frac{d[PH_3]}{dt}=\frac{1}{4}\times 0.002042 M/s=0.0005105 M/s](/tpl/images/0405/9326/7d03f.png)
:![R=\frac{1}{1}\frac{d[P_4]}{dt}](/tpl/images/0405/9326/34938.png)
![\frac{d[P_4]}{dt}=\frac{1}{1}\times 0.0005105 M/s=0.0005105 M/s](/tpl/images/0405/9326/4315e.png)
:![R=\frac{1}{6}\frac{d[P_4]}{dt}](/tpl/images/0405/9326/3100b.png)
![\frac{d[H_2]}{dt}=\frac{6}{1}\times 0.0005105 M/s=0.003063 M/s](/tpl/images/0405/9326/b8130.png)
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Consider the reaction 4 ph3(g) → p4(g) + 6 h2(g). if, in a certain experiment, over a specific time...
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