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It can be + or - depending on the value of the entropy (∆S). Recall, that ∆G = ∆H - T∆S and for a spontaneous reaction, ∆G must be negative, so you can see how this will depend on the values and signs of both enthalpy and entropy.
A standard, as in the standard values of weights and measures.
the values you actually get when you do the procedure, these are then compared to the standard values
To compare the atomic mass and rf values with the standard
The platinum black provides a very high surface area that promotes the speed of reaction at the electrode and thereby virtually eliminates overpotential at the standard hydrogen electrode. An overpotential would lead to misleading values of potential of other electrodes compared with a standard hydrogen electrode that manifested overpotential.
It can be + or - depending on the value of the entropy (∆S). Recall, that ∆G = ∆H - T∆S and for a spontaneous reaction, ∆G must be negative, so you can see how this will depend on the values and signs of both enthalpy and entropy.
entropy is greater the more possible arrangements for energy there are, which increases as the molecules become more mobile, so entropy is high in a gas, lower in a liquid, and lowest in a solid.
For data sets having a normal, bell-shaped distribution, the following properties apply: About 68% of all values fall within 1 standard deviation of the mean About 95% of all values fall within 2 standard deviation of the mean About 99.7% of all values fall within 3 standard deviation of the mean.
Relationship between values goals and standard
carbon resistors of standard values are manufactured because other values can be obtained by series and parallel combination of standard values. Moreover even standard values do not offer exact Resistance's will have tolerance
the values you actually get when you do the procedure, these are then compared to the standard values
A standard, as in the standard values of weights and measures.
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When the two denominator values in the eclipse standard equation are the same, it can be said to be in foci.
0111 0110
When H2O(l) evaporates to H2O(g), hydrogen bonds are broken and energy is absorbed. This means it is endothermic. To go from liquid to gas, entropy needs to increase because gas has more disorder, which means a change in entropy (ΔS) should be positive. ΔG = ΔH - TΔS, so when ΔG is negative the reaction is spontaneous. For ΔG to be negative TΔS should be greater than ΔH. This can be shown mathematically (e.g. T is equal to 373.15 and the values of ΔS and ΔH can be calculated) and thus the evaporation of H2O is spontaneous.
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