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For the reaction N(2)(g)+3" H"(2)(g)to2"...

For the reaction `N_(2)(g)+3" H"_(2)(g)to2" NH"_(3)(g)`, if
`Delta[NH_(3)]//Deltat=4xx10^(-8)" mol L"^(-1)s^(-1)` what is the value of `-Delta[H_(2)]//Deltat` ?

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AI Generated Solution

To solve the problem, we need to determine the rate of disappearance of \( H_2 \) given the rate of formation of \( NH_3 \) for the reaction: \[ N_2(g) + 3 H_2(g) \rightarrow 2 NH_3(g) \] ### Step-by-Step Solution: 1. **Identify the stoichiometry of the reaction**: The balanced equation tells us that 1 mole of \( N_2 \) reacts with 3 moles of \( H_2 \) to produce 2 moles of \( NH_3 \). This means that for every 2 moles of \( NH_3 \) produced, 3 moles of \( H_2 \) are consumed. ...
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