when two protons are put togehter alone.
The lattice energy of a compound is always negative.
No, binding energy cannot be negative. Binding energy is always a positive quantity that represents the energy required to hold a system together. If the binding energy were negative, it would imply that the system is in an unstable state.
Yes, the change in kinetic energy can be negative if the object's speed decreases, resulting in a decrease in kinetic energy.
No, the lattice energy can be positive, negative, or zero, depending on the specific compounds involved.
Yes, it is possible for the change in kinetic energy to be negative. This occurs when an object loses kinetic energy, such as when it slows down or comes to a stop.
The enthalpy change of combustion is always negative because it involves the breaking of bonds in the reactants, which requires energy input, and the formation of new bonds in the products, which releases energy. The energy released during bond formation is greater than the energy required for bond breaking, resulting in a net release of energy, hence the negative value.
The lattice energy of a compound is always negative.
No, binding energy cannot be negative. Binding energy is always a positive quantity that represents the energy required to hold a system together. If the binding energy were negative, it would imply that the system is in an unstable state.
Yes, the change in kinetic energy can be negative if the object's speed decreases, resulting in a decrease in kinetic energy.
No, a process with a large negative g does not always proceed rapidly. The rate of a reaction is determined by various factors, not just the change in free energy.
bcoz the energy of bound system is always negative
Gibbs free energy (ΔG) will always be negative for a spontaneous process occurring at constant temperature and pressure. This typically occurs when the change in enthalpy (ΔH) is negative (exothermic reactions) and the change in entropy (ΔS) is positive, leading to a favorable increase in disorder. Additionally, even if ΔH is positive, a sufficiently large positive change in entropy can also result in a negative ΔG at high temperatures, according to the equation ΔG = ΔH - TΔS.
No, the lattice energy can be positive, negative, or zero, depending on the specific compounds involved.
Yes, it is possible for the change in kinetic energy to be negative. This occurs when an object loses kinetic energy, such as when it slows down or comes to a stop.
A reaction is always spontaneous when the change in Gibbs free energy (ΔG) is negative (ΔG < 0). This occurs when the system's enthalpy change (ΔH) is negative and the entropy change (ΔS) is positive, or when the temperature is sufficiently low to make the term TΔS (where T is temperature) less significant compared to ΔH. In summary, spontaneous reactions can be identified by a negative ΔG value, indicating that they can occur without external input.
The hydration of an ion is negative because energy is released when water molecules surround and stabilize the ion. This release of energy is favorable and results in a negative enthalpy change. The hydration process is exothermic, meaning it releases heat.
when H is negative and S is positive