Thermodynamics
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Which of the following statements is correct?
(i) The presence of reacting species in a covered beaker is an example of open system.
(ii) There is an exchange of energy as well as matter between the system and the surroundings in a closed system.
(iii) The presence of reactants in a closed vessel made up of copper is an example of a closed system.
(iv) The presence of reactants in a thermos flask or any other closed insulated vessel is an example of a closed system.
Which of the following statements is correct?
(i) The presence of reacting species in a covered beaker is an example of open system.
(ii) There is an exchange of energy as well as matter between the system and the surroundings in a closed system.
(iii) The presence of reactants in a closed vessel made up of copper is an example of a closed system.
(iv) The presence of reactants in a thermos flask or any other closed insulated vessel is an example of a closed system.
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (iii)
The presence of reactants in a closed vessel made of conducting material e.g., copper or steel is an example of a closed system.
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Thermodynamics is not concerned about______.
(i) Energy changes involved in a chemical reaction.
(ii) The extent to which a chemical reaction proceeds.
(iii) The rate at which a reaction proceeds.
(iv) The feasibility of a chemical reaction.
Thermodynamics is not concerned about______.
(i) Energy changes involved in a chemical reaction.
(ii) The extent to which a chemical reaction proceeds.
(iii) The rate at which a reaction proceeds.
(iv) The feasibility of a chemical reaction.
This is a Multiple Choice Questions as classified in NCERT Exemplar
Thermodynamics is not concerned about how and at what rate these energy transformations are carried out but is based on initial and final states of a system undergoing the change. Laws of thermodynamics apply only when a system is in
Upvote An ideal gas is allowed to expand against a constant pressure of 2 bar from 10 L to 50 L in one step. Calculate the amount of work done by the gas. If the same expansion were carried out reversibly, will the work done be higher or lower than the earlier case?
An ideal gas is allowed to expand against a constant pressure of 2 bar from 10 L to 50 L in one step. Calculate the amount of work done by the gas. If the same expansion were carried out reversibly, will the work done be higher or lower than the earlier case?
This is a Short Answer Type Questions as classified in NCERT Exemplar
We know that the amount of work done =-pext? V
On substituting the values in the formula, we get,
-2bar* (50-10)L=-80Lbar
According to the described problem,1 LBar = 100J
Therefore, -80 L bar= (-80*100)= -8000J
= -8kJ, which is the amo
Upvote 1.0 mol of a monoatomic ideal gas is expanded from state (1) to state (2) as shown in Fig. 6.4. Calculate the work done for the expansion of gas from state (1) to state (2) at 298 K.
1.0 mol of a monoatomic ideal gas is expanded from state (1) to state (2) as shown in Fig. 6.4. Calculate the work done for the expansion of gas from state (1) to state (2) at 298 K.
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We can conclude from the figure that this change is a reversible change.
Now,
W= -2.303nRT log
But, p1V1 = p2V2 = = = =2
W= -2.303nRT log
= -2.303 *8.314*1*298*log2
= -2.303 *8.314*298*0.3010J
= -1717.46J
Upvote Enthalpy diagram for a particular reaction is given in Fig. 6.3. Is it possible to decide spontaneity of a reaction from given diagram. Explain
Enthalpy diagram for a particular reaction is given in Fig. 6.3. Is it possible to decide spontaneity of a reaction from given diagram. Explain
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No, for the state of spontaneity, the enthalpy change is not the only criteria. Entropy also needs to be taken into account here.
Upvote Represent the potential energy/enthalpy change in the following processes graphically.
(a) Throwing a stone from the ground to roof.
(b) 12H2(g) + 12Cl2(g) HCl(g) ?rH? = –92.32 kJ/ mol
In which of the processes potential energy/enthalpy change is contributing factor to the spontaneity?
Represent the potential energy/enthalpy change in the following processes graphically.
(a) Throwing a stone from the ground to roof.
(b) 12H2(g) + 12Cl2(g) HCl(g) ?rH? = –92.32 kJ/ mol
In which of the processes potential energy/enthalpy change is contributing factor to the spontaneity?
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Throwing a stone from ground to roof
b) the reaction involved is a process where the energy decreases after the reaction. It can be represented as:In process b), potential energy/enthalpy change is a contributing factor to the spont
Upvote How will you calculate work done on an ideal gas in a compression, when change in pressure is carried out in infinite steps ?
How will you calculate work done on an ideal gas in a compression, when change in pressure is carried out in infinite steps ?
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When a process can be reversed by bringing an extremely small change in it, we call it a reversible process. The pressure-volume graph can be used to calculate the work done. The pressure is not constant, and changes in infinitesim
Upvote What will be the work done on an ideal gas enclosed in a cylinder, when it is compressed by a constant external pressure, pext in a single step as shown in Fig. 6.2. Explain graphically
What will be the work done on an ideal gas enclosed in a cylinder, when it is compressed by a constant external pressure, pext in a single step as shown in Fig. 6.2. Explain graphically
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Assumption: Cylinder is filled with one mole gas, and the piston is frictionless. Let the pressure of gas inside be p and the volume of gas be V_ {I}.
Piston is moved towards the inside to make the external pressure (P_ {ext}) equal
Upvote The enthalpy of reaction for the reaction : 2H2(g) + O2(g) → 2H2O(l) is ∆rHᶱ = – 572 kJ/ mol. What will be standard enthalpy of formation of H2O (l ) ?
The enthalpy of reaction for the reaction : 2H2(g) + O2(g) → 2H2O(l) is ∆rHᶱ = – 572 kJ/ mol. What will be standard enthalpy of formation of H2O (l ) ?
Chemistry NCERT Exemplar Solutions Class 11th Chapter six
Standard molar enthalpy of formation is the enthalpy change for the formation of one mole of a compound from its most stable states or reference states. As per the given information in the question, the standard enthalpy for the given eq
Upvote The enthalpy of vapourisation of CCl4 is 30.5 kJ/ mol. Calculate the heat required for the vapourisation of 284 g of CCl4 at constant pressure. (Molar mass of CCl4 = 154 g/mol).
The enthalpy of vapourisation of CCl4 is 30.5 kJ/ mol. Calculate the heat required for the vapourisation of 284 g of CCl4 at constant pressure. (Molar mass of CCl4 = 154 g/mol).
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As per the information provided in the question, for one mole of CCl4 (154 g), the heat of vaporisation required is 30.5 kJ/mol .
Hence for the vaporisation of 284 g of CCl4, we require:
= 56.2 kJ
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