Chemistry, 26.03.2020 22:01, kharmaculpepper
Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of disappearance of Cl2 is 4.44 × 10-2 M/s, what is the rate of disappearance of NO? 2 NO(g) + Cl2(g) → 2 NOCl(g) Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of disappearance of Cl2 is 4.44 × 10-2 M/s, what is the rate of disappearance of NO? 2 NO(g) + Cl2(g) → 2 NOCl(g) 2.22 × 10-2 M/s 1.11 × 10-1 M/s 4.44 × 10-2 M/s 8.88 × 10-2 M/s 5.25 × 10-2 M/s
Answers: 3
![-\frac{1d[NO]}{2dt}=-\frac{d[Cl_2]}{dt}=+\frac{1d[NOCl]}{2dt}](/tpl/images/0565/9272/04d4d.png)
![\frac{-d[Cl_2]}{dt}]=4.44\times 10^{-2}M/s](/tpl/images/0565/9272/271c7.png)
![-\frac{1d[NO]}{dt}=2\times {\frac{-d[Cl_2]}{dt}=2\times 4.44\times 10^{-2}M/s=8.88\times 10^{-2}M/s](/tpl/images/0565/9272/dea34.png)
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Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the...
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