- The problem follows the law of conservation of mass, which states the total mass of reactants equals the total mass of products in a complete reaction.
- Colin combines \(10\) g of substance \(A\) and \(45\) g of substance \(B\).
- Assuming complete consumption of reactants, the total mass of the product \(AB\) is \(10 \text{ g} + 45 \text{ g} = 55 \text{ g}\).
- The final answer is \(\boxed{55 \text{ g}}\).
Explanation
- Analyzing the Chemical Reaction and Conservation of Mass
The chemical reaction described is \(A + B \rightarrow AB\), which follows the law of conservation of mass. This law states that in any closed system, the mass of the substances involved in a reaction remains constant; therefore, the total mass of the products must equal the total mass of the reactants consumed. Colin combines \(10\) g of substance \(A\) and \(45\) g of substance \(B\). In basic stoichiometry problems where no specific molar masses or limiting reagents are provided, it is typically assumed that the reactants are completely consumed to form the product, provided the reaction can occur. Thus, the mass of the product \(AB\) formed is the sum of the masses of the reactants \(A\) and \(B\).
- Calculating the Mass of Product AB
Given that Colin adds \(10\) g of substance \(A\) and \(45\) g of substance \(B\), we calculate the total mass of the reactants as:
\[\text{Total mass} = \text{mass}(A) + \text{mass}(B) = 10 \text{ g} + 45 \text{ g} = 55 \text{ g}.\]
According to the law of conservation of mass, if both reactants are fully consumed in the reaction \(A + B \rightarrow AB\), the total mass of the product \(AB\) will be equivalent to the combined mass of the reactants. Therefore, the total amount of substance \(AB\) produced is \(55\) g.
- Conclusion
Comparing our calculated total mass with the provided options (\(10\) g, \(35\) g, \(45\) g, \(55\) g), the result \(55\) g matches perfectly with the principle of complete consumption of reactants in this stoichiometric scenario. Thus, Colin will make \(55\) g of substance \(AB\). Consequently, the final answer is \(\boxed{55 \text{ g}}\).
Examples
In a professional laboratory setting, chemists use the law of conservation of mass to predict the yield of a reaction. For example, if you are synthesizing a compound for a pharmaceutical study by mixing \(50\) mg of a precursor and \(120\) mg of a catalyst, you can determine that the theoretical mass of your output (assuming total reaction) is \(50 \text{ mg} + 120 \text{ mg} = 170 \text{ mg}\). This principle is fundamental for verifying the efficiency of chemical processes and ensuring that no materials are lost during synthesis.