This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Step 1: Assign variables to the stoichiometric coefficients for each reactant and product. Let a, b, and c be the coefficients for Fe, Cl_2, and FeCl_3 respectively. aFe + bCl_2 → cFeCl_3 Step 2: Write down the balance equations for each element present in the reaction. For Iron (Fe): The number of Fe atoms on the reactant side must equal the number of Fe atoms on the product side. a = c (1) For Chlorine (Cl): The number of Cl atoms on the reactant side must equal the number of Cl atoms on the product side. 2b = 3c (2) Step 3: Assign a value to one of the variables to solve the system of equations. Let's assume a = 1. Step 4: Solve for the other variables using the equations. From equation (1): If a = 1, then c = 1. Substitute c = 1 into equation (2): 2b = 3(1) 2b = 3 b = (3)/(2) Step 5: Convert fractional coefficients to whole numbers. The coefficients are a=1, b=(3)/(2), c=1. To get whole numbers, multiply all coefficients by the smallest integer that eliminates the fraction, which is 2. a = 1 × 2 = 2 b = (3)/(2) × 2 = 3 c = 1 × 2 = 2 Step 6: Write the balanced chemical equation using the whole number coefficients. 2Fe + 3Cl_2 → 2FeCl_3 The balanced equation is: 2Fe + 3Cl_2 → 2FeCl_3 Send me the next one 📸