Identify the total number of moles involved in the reaction: 2C_(4)H_(10)(g)+13O_(2)(g)arrow 10H_(2)O(g)+8CO_(2)(g) 33 15 18 4

Answer:# Explanation: ## Step 1: Understanding the Chemical ReactionThe given problem is a balanced chemical equation, which represents the combustion reaction of Butane (C4H10) with Oxygen (O2). This reaction results in the formation of Water (H2O) and Carbon Dioxide (CO2).## Step 2: Identifying the Mole RatiosThe coefficients in front of the chemical formulas in a balanced chemical equation represent the mole ratios of the reactants and products. In this case, the coefficients are 2 for Butane, 13 for Oxygen, 10 for Water, and 8 for Carbon Dioxide.## Step 3: Calculating the Total MolesThe total number of moles involved in the reaction can be calculated by adding the number of moles of each reactant and product. In this case, there are 2 moles of Butane, 13 moles of Oxygen, 10 moles of Water, and 8 moles of Carbon Dioxide involved in the reaction.### **Total Moles Involved = Moles of Butane + Moles of Oxygen + Moles of Water + Moles of Carbon Dioxide**### **Total Moles Involved = 2 + 13 + 10 + 8 = 33 moles**## Step 4: Verifying the Law of Conservation of MassThis calculation reflects the law of conservation of mass, which states that in a closed system, the total mass of the reactants is equal to the total mass of the products. This is because matter is neither created nor destroyed in a chemical reaction.# Answer:The total number of moles involved in the given reaction is '33'.