Answer:
V = 48.5 L
Explanation:
Converting °C to K and kPa to atm
T = 25.0°C + 273.15 = 298.15 K
P = 61.3 kPa × (1 atm / 101.325 kPa) = 0.60498 atm
Calculating the volume of gas
V = nRT / P
V = (1.20 mol)(0.082057 L•atm/mol•K)(298.15 K) / 0.60498 atm
V = 48.5 L
Answer:
The correct answer is B. It is spontaneous only at low temperatures.
Explanation:
In thermodynamics, the Gibbs free energy is a thermodynamic potential that can be used to calculate the maximum of reversible work that may be performed by a thermodynamic system at a constant temperature and pressure.
The spontaneity of a reaction is given by the equation:
ΔG = ΔH - TΔS
where:
ΔH: enthalpy variation
T: absolute temperature
ΔS: entropy variation
As the reaction is exothermic, ΔH<0
As the reaction order increases (the reagents are solid and gas and their product is solid), ΔS<0
Therefore, the reaction will be spontaneous when ΔG is negative.
ΔG = ΔH - TΔS
That is, the entropy term must be smaller than the enthalpy term.
Hence, the reaction will be spontaneous only at low temperatures.
Well i do think they're the same.
5.4 M = moles of solute / 1.50 L
<span>Multiply both sides by 1.50 L to isolate moles of solute on the right. </span>
<span>8.1 mol = moles of solute </span>
Answer:
Immiscible
Explanation:
Not sure what kind of substance but this is form liquids.