Balance the following reaction A coefficient of "1"is understood. Choose option "blank" for the correct answer if the coefficient is "1." NH_(3)+ +F_(2)arrow FN_(2)F_(4)+

To balance the chemical equation, we need to ensure that the number of each type of atom on the reactant side is equal to the number on the product side.<br /><br />The unbalanced equation is:<br /><br />\[ NH_3 + F_2 \rightarrow FN_{2}F_{4} + \]<br /><br />Let's break it down:<br /><br />1. **Nitrogen (N):** <br /> - Reactants: 1 nitrogen in \(NH_3\)<br /> - Products: 2 nitrogens in \(FN_{2}F_{4}\)<br /><br /> To balance nitrogen, we need 2 \(NH_3\):<br /><br /> \[ 2NH_3 + F_2 \rightarrow FN_{2}F_{4} + \]<br /><br />2. **Fluorine (F):** <br /> - Reactants: \(F_2\) provides 2 fluorines per molecule.<br /> - Products: 6 fluorines in \(FN_{2}F_{4}\)<br /><br /> To balance fluorine, we need 3 \(F_2\):<br /><br /> \[ 2NH_3 + 3F_2 \rightarrow FN_{2}F_{4} + \]<br /><br />3. **Hydrogen (H):** <br /> - Reactants: 6 hydrogens from 2 \(NH_3\)<br /> - Products: No hydrogen in \(FN_{2}F_{4}\), so we need to add 3 \(H_2\) as a product to balance hydrogen:<br /><br /> \[ 2NH_3 + 3F_2 \rightarrow FN_{2}F_{4} + 3H_2 \]<br /><br />Now, the balanced equation is:<br /><br />\[ 2NH_3 + 3F_2 \rightarrow FN_{2}F_{4} + 3H_2 \]<br /><br />So the coefficients are:<br />- \(NH_3\): 2<br />- \(F_2\): 3<br />- \(FN_{2}F_{4}\): 1 (choose "blank" for this option)<br />- \(H_2\): 3