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At 800^(@)C the rate of reaction 2NO + H...

At `800^(@)C` the rate of reaction `2NO + H_(2) rarr N_(2) + H_(2)O` Changes with the concentration of `NO and H_(2)` are
[NO] in M`" "[H_(2)]" in M "" "-(1)/(2) (d[NO])/(dt)" in M sec"^(-1)`
(i) `1.5xx10^(-4)" "4xx10^(-3)" "4.4xx10^(-4)`
(ii) `1.5xx10^(-4)" "2xx10^(-3)" "2.2xx10^(-4)`
(iii) `3.0xx10^(-4)" "2xx10^(-3)" "8.8xx10^(-4)`
(a) What is the order of this reaction ?
(b) What is the rate equation for the reaction ?
(c) What is the rate when
`[H_(2)]=1.5xx10^(-3)" M and "[NO]=1.1xx10^(-3) M` ?

Text Solution

Verified by Experts

(a) Third order, (b) `r=k [NO]^(2)[H_(2)]`, (c ) `8.85xx10^(-3)" M sec"^(-1)`
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