Answer:
<em><u>When ΔS > 0 and ΔH < 0, the process is always spontaneous as written. When ΔS < 0 and ΔH > 0, the process is never spontaneous, but the reverse process is always spontaneous. When ΔS > 0 and ΔH > 0, the process will be spontaneous at </u></em>
Explanation:
What are the best conditions to lead towards a spontaneous reaction? <em><u>high negative enthalpy, high temp, high positive entropy. Your enthalpy is high and negative but your entropy is also negative.</u></em>
Many times, solutions lie between two quantities, rather than continuing endlessly in one direction. For example systolic (top number) blood pressure that is between 120 and 139 mm Hg is called borderline high blood pressure. This can be described using a compound inequality, b < 139 and b > 120. Other compound inequalities are joined by the word “o
Explanation:
Gay-Lussac's law states that the pressure of a given mass of gas varies directly with the absolute temperature of the gas when the volume is kept constant. Mathematically, it can be written as: {\displaystyle {\frac {P}{T}}=k}. It is a special case of the ideal gas law.
<span>There
are a number of ways to express concentration of a solution. This includes
molarity and molality. Molarity is expressed as the number of moles of solute per volume of
the solution. MOlality is expressed as moles per kg solution.
5.25 mol H2SO4 / kg solution ( 1 kg / 1000 g ) ( 1.266 g / mL ) ( 1000 mL / 1L ) = 6.6 M H2SO4</span>
Hello! Your answer would be a gain of electrons and a decrease in positive charge.
Contrary to how it sounds, reduction is actually a gain of electrons. It is part of a set of reactions known as a redox reaction, reduction being a gain of electrons and oxidation being a loss.
With the gain of electrons, the element would become more negative as electrons bring with them a negative charge. Therefore, this would decrease the positive charge.
Hope this helped!
