Advertisements
Advertisements
प्रश्न
In which of the following, entropy of the system decreases?
पर्याय
Crystallization of liquid into solid.
Temperature of crystalline solid is increased from 0 K to 115 K
H2(g) → 2H(g)
2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g)
Advertisements
उत्तर
Crystallization of liquid into solid
Explanation:
- A system's disorder or difficulty is measured by its entropy.
- A liquid turns into a solid—a more ordered state—during the crystallisation process.
- Because the particles become more organised and have less mobility, entropy consequently falls.
APPEARS IN
संबंधित प्रश्न
Define entropy.
Answer the following in one or two sentences.
State second law of thermodynamics in terms of entropy.
For a certain reaction ΔH° = 219 kJ and ΔS° = –21 J/K. Determine whether the reaction is spontaneous or nonspontaneous.
Identify the INCORRECT statement.
For a process, entropy change of a system is expressed as ________.
For a reversible spontaneous change, ∆S is ____________.
Arrange the following in order of increasing entropy.
I. 1.0 mol H2O (298 K, 1 atm)
II. 1.0 mol H2O (270 K, 1 atm)
III. 1.0 mol H2O (400 K, 1 atm)
In which of the following, ∆S is positive?
Which one of the following has ΔS0 greater than zero?
For the following reaction:
\[\ce{Fe2O3_{(s)} + 3CO_{(g)} -> 2Fe_{(s)} + 3CO2_{(g)}}\]; ΔH0 = −29.8 kJ and ΔS0 = 15 J K−1. What is the value of \[\ce{ΔS_{(total)}}\] at 298 K?
Which of the following conditions indicates the reaction is spontaneous?
For a reaction to be non-spontaneous at all temperatures, values of ΔH and ΔS respectively are ____________.
If ΔH° and ΔS° for the reaction \[\ce{N2O_{4(g)} -> 2NO_{2(g)}}\] is 57.24 kJ and 175.8 JK-1 mol-1 respectively. What is the value of ΔG° for this reaction at 298 K?
Standard molar entropy is ______.
Calculate the amount of heat liberated during formation of 2. 7 kg of water if heat of formation of water is - 284.5 kJ mol-1.
A reaction is spontaneous at low temperatures but non-spontaneous at high temperatures. Which of the following is true for the reaction?
The criterion for a spontaneous process is ______.
Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are −382.64 kJ mol−1 and −145.6 JK−1 mol−1, respectively. Standard Gibb's energy change for the same reaction at 298 K is ______.
In which of the following reaction the value of Kp will be equal to Kc?
Dinitrogen and dioxygen combined to form nitrous oxide in equilibrium at 850 K. The equilibrium constant for this reaction is 0.56. If the equilibrium concentration of nitrous oxide gas is 3 × 10-3 M and both dinitrogen and dioxygen have the same concentration, then what will be the concentration of dinitrogen gas in M?
Identify whether the following pair have larger entropy or not. If yes then Why?
He(g) in a volume of 1 L or He(g) in a volume of 5 L both at 25°C.
Write the relationship between Gibbs energy change for a process and total entropy change of system and surroundings.
ΔH for the reaction is − 110 kJ, and ΔS is + 40 JK−1 at 400 K. The free energy change for the reaction is ______.
For a certain reaction ΔH0 is −224 kJ and ΔS0 is −153 J K−1. At what temperature the change over from spontaneous to non-spontaneous will occur?
