A student adds a 3.0 g antacid tablet to 35.0 g of water in a bottle. After the reaction is complete, 37.3 g of liquid remains in the bottle. How much gas was formed in the reaction?
A. 0.7 g
B. 2.3 g
C. 3.0 g
D. 75.3 g

A.  0.7 g

Explanation:

According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.

antacid + water  →  liquid + gas

 3.0 g  + 35.0 g   = 37.3 g + x

38.0 g = 37.3 + x

x = 38.0 g - 37.3 g

x = 0.7 g

This law was given by French chemist  Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.

For example:

In given photosynthesis reaction:

6CO₂ + 6H₂O + energy → C₆H₁₂O₆ + 6O₂

there are six carbon atoms, eighteen oxygen atoms and twelve hydrogen atoms on the both side of equation so this reaction followed the law of conservation of mass.

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explanation:

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.