2026.8378 I might get it wrong but I’m pretty sure it’s right
Answer:
1. d. The reaction is spontaneous in the reverse direction at all temperatures.
2. c. The reaction is spontaneous at low temperatures.
Explanation:
The spontaneity of a reaction is associated with the Gibbs free energy (ΔG). When ΔG < 0, the reaction is spontaneous. When ΔG > 0, the reaction is non-spontaneous. ΔG is related to the enthalpy (ΔH) and the entropy (ΔS) through the following expression:
ΔG = ΔH - T. ΔS [1]
where,
T is the absolute temperature (T is always positive)
<em>1. What can be said about an Endothermic reaction with a negative entropy change?</em>
If the reaction is endothermic, ΔH > 0. Let's consider ΔS < 0. According to eq. [1], ΔG is always positive. The reaction is not spontaneous in the forward direction at any temperature. This means that the reaction is spontaneous in the reverse direction at all temperatures.
<em>2. What can be said about an Exothermic reaction with a negative entropy change?</em>
If the reaction is exothermic, ΔH < 0. Let's consider ΔS < 0. According to eq. [1], ΔG will be negative when |ΔH| > |T.ΔS|, that is, at low temperatures.
Answer: (D.) Planting Roof gardens
Explanation: I'm really hoping you get this right but the reason of my answer is because Trees, green roofs, and vegetation can help reduce urban heat island effects by shading building surfaces, deflecting radiation from the sun, and releasing moisture into the atmosphere.
An indicator shows where the endpoint of a titration is. Different indicators will change colors at different equivalence points. Phenolphthalein will change colors at around pH7.5 or so, and others like Methylene Blue will change around a pH of 6. Different titrations will have different pH's at different equivalence points.
Decreasing the volume increases the pressure, therefore due to Le Chatelier's principle, we can see that more HI2 will be formed as 2 molecules combine into 1 and that conserves space which in turn lowers the pressure.
