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50.0 kg of N(2) (g) and 10 g of H(2) (g)...

`50.0 kg` of `N_(2) (g)` and `10 g` of `H_(2) (g)` are mixed to produce `NH_(3) (g)`. Calculate the `NH_(3) (g)` formed. Identify the limiting reagent.

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To solve the problem of calculating the amount of ammonia (NH₃) formed from the reaction of nitrogen (N₂) and hydrogen (H₂), we will follow these steps: ### Step 1: Write the Balanced Chemical Equation The balanced chemical equation for the formation of ammonia is: \[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \] ### Step 2: Calculate the Moles of Reactants We need to calculate the number of moles of N₂ and H₂ using their given masses and molar masses. ...
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