For a reaction to be nonspontaneous under standard conditions at all temperatures, the signs of ΔH and ΔS must be positive and negative, respectively.
<span>Gibbs free energy
(G) determines if reaction will proceed spontaneously.
</span><span>ΔG = ΔH - T·ΔS.</span>
ΔG - changes in Gibbs
free energy.<span>
ΔH - changes in enthalpy.
ΔS - changes in entropy.
T is temperature in Kelvins.
When ΔS < 0 (negative entropy change) and
ΔH > 0 (endothermic reaction), the process is never spontaneous (<span>ΔG> 0).
</span></span>
Answer:
c
Explanation:
the way you move explains how confident you are
Answer: F. Electrons
Explanation: hope it helped .u.
Answer:
Final volume=V₂ = 216.3 mL
Explanation:
Given data:
Initial volume = 120.0 mL
Initial temperature = -12.3 °C (-12.3 +273 = 260.7 K)
Final volume = ?
Final temperature = 197.0 °C (197+273 = 470 K)
Solution:
We will apply Charles Law to solve the problem.
According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.
Mathematical expression:
V₁/T₁ = V₂/T₂
V₁ = Initial volume
T₁ = Initial temperature
V₂ = Final volume
T₂ = Final temperature
Now we will put the values in formula.
V₁/T₁ = V₂/T₂
V₂ = V₁T₂/T₁
V₂ = 120 mL × 470 K /260.7K
V₂ = 56400 mL.K /260.7K
V₂ = 216.3 mL
