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Photosynthesis is the process by which plants and other organisms convert carbon dioxide and water into glucose and oxygen using light energy. The general reaction for photosynthesis can be represented as follows: 6 CO鈧� (g) + 6 H鈧侽 (l) + light energy 鈫� C鈧咹鈧佲倐O鈧� (s) + 6 O鈧� (g)

Entropy is a measure of the molecular disorder, or randomness in a system. During the photosynthesis process, reactants (CO鈧� and H鈧侽) are converted into products (glucose and O鈧�). Considering the phases of reactants and products, we notice that there is a decrease in the number of moles of gaseous substance, and a solid substance (glucose) is formed. The process leads to an overall decreased randomness, so the change in entropy for the system (\(\Delta S_{\mathrm{sy}}\)) should be negative. Thus, \(\Delta S_{\mathrm{sy}} < 0\).

For an endothermic process, heat is absorbed from the surroundings, and the local environment becomes colder. In the case of photosynthesis, light energy from the sun is absorbed to convert CO鈧� and H鈧侽 molecules into glucose and O鈧�. Hence, photosynthesis is an endothermic process. As heat is absorbed from the surroundings to perform the reaction, this causes an increase in entropy for the surroundings. We can then say that the change in entropy for the surroundings (\(\Delta S_{\mathrm{su}}\)) is positive. Thus, \(\Delta S_{\mathrm{su}} > 0\).

To determine the change in entropy for the universe, we need to consider both the system and the surroundings. By the second law of thermodynamics, the total entropy change is the sum of the entropy change of the system and the entropy change of the surroundings: \(\Delta S_{\text{univ}} = \Delta S_{\mathrm{sy}} + \Delta S_{\mathrm{su}}\) Given that \(\Delta S_{\mathrm{sy}} < 0\) (negative) and \(\Delta S_{\mathrm{su}} > 0\) (positive), the signs of \(\Delta S_{\mathrm{sy}}\) and \(\Delta S_{\mathrm{su}}\) are opposite. Therefore, without knowing the exact numerical values, we cannot definitively determine the sign of \(\Delta S_{\text{univ}}\). In conclusion: - The change in entropy for the system (\(\Delta S_{\mathrm{sy}}\)) is negative: \(\Delta S_{\mathrm{sy}} < 0\). - The change in entropy for the surroundings (\(\Delta S_{\mathrm{su}}\)) is positive: \(\Delta S_{\mathrm{su}} > 0\). - The change in entropy for the universe (\(\Delta S_{\text {univ }}\)) cannot be definitively determined without knowing the exact numerical values: \(\Delta S_{\text{univ}} = \Delta S_{\mathrm{sy}} + \Delta S_{\mathrm{su}}\) (negative, positive, or zero).