Fiber optic cable structure illustrating light propagation within the core and cladding layers.

Let’s solve this step by step.

We are given a chemical reaction:

Glucose + Oxygen → Carbon Dioxide + Water + Energy

And we’re told that in an experiment, 180 grams of glucose and 192 grams of oxygen were used. The products were 264 grams of carbon dioxide and some amount of water (which we need to find), plus energy.

Also, we’re reminded of the Law of Conservation of Mass:
> Matter cannot be created or destroyed in a chemical reaction. So, the total mass of reactants = total mass of products.

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Step 1: Add up the mass of the reactants

Reactants = Glucose + Oxygen
= 180 g + 192 g
= 372 grams

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Step 2: Add up the known mass of the products

Products = Carbon Dioxide + Water + Energy

But note: Energy does not have mass — it’s not matter. So we ignore it when adding masses.

So far, we know:
- Carbon Dioxide = 264 g
- Water = ? (let’s call it W)

Total product mass = 264 g + W

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Step 3: Set up equation using conservation of mass

Mass of reactants = Mass of products
372 g = 264 g + W

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Step 4: Solve for W (mass of water)

W = 372 - 264
W = 108 grams

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✔ Double-check:
Reactants: 180 + 192 = 372 g
Products: 264 (CO₂) + 108 (H₂O) = 372 g
Yes! It balances.

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Final Answer:
108 grams