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11th
Chemistry
Thermodynamics
$Internal Energy as a State of System$

Internal Energy as a State of System

Thermodynamics

Chemistry

Class 11

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Internal Energy and the First Law of Thermodynamics

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Thermodynamics : Videos, Concepts, Examples, Heat, Work and Energy Thermodynamic Terms: Heat, Temperature, Open/Closed System & so on NCERT Solutions for Class 11 Chemistry Chapter 6 Free PDF Download

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Heat as Internal Energy

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First Law of Thermodynamics

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First Law of Thermodynamics

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Internal Energy

ExampleDefinitionsFormulaes

For which of the following reaction $△ H = △ E + 2 R T$

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Assertion (A) : Zeroth law of thermodynamics gives us the concept of energy
Reason (R) : Internal energy is dependent on temperature

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One gram of water on evaporation at atmospheric pressure forms $1671 c m^{3}$ of steam. The heat of vaporisation at this pressure is $540 c a l / g m$ . The increase in internal energy is

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Energy hidden in a definite quantity of substance is:

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The reaction between $Δ G$ and $Δ H$ is:

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Which of the following statements are correct as per IUPAC sign convention?

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According to the first law of thermodynamics, $Δ U = q + w$ . In special cases the statement can be expressed in different ways. Which of the following is not a correct expression?

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The change in internal energy of the methanol is

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For the reaction $C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l)$ the difference between enthalpy change and internal energy change is:

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Assuming that water vapour is an ideal gas, the internal energy change $(Δ U)$ when $1 m o l$ of water is vapourised at $1 b a r$ pressure and $10 0^{\circ} C .$ (Given: Molar enthalpy of vapourisation of water at $1 b a r$ and $373 K = 41 k J m o l^{- 1}$ and $R = 8.3 J m o l^{- 1} K^{- 1} will be)$

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Internal Energy as a State of System

Overview

Learn

Videos

Study Materials

Quick summary with Stories

Heat as Internal Energy

First Law of Thermodynamics

Revise with Concepts

First Law of Thermodynamics

Internal Energy

Related questions

For which of the following reaction $△ H = △ E + 2 R T$

Assertion (A) : Zeroth law of thermodynamics gives us the concept of energy
Reason (R) : Internal energy is dependent on temperature

One gram of water on evaporation at atmospheric pressure forms $1671 c m^{3}$ of steam. The heat of vaporisation at this pressure is $540 c a l / g m$ . The increase in internal energy is

Energy hidden in a definite quantity of substance is:

The reaction between $Δ G$ and $Δ H$ is:

Which of the following statements are correct as per IUPAC sign convention?

According to the first law of thermodynamics, $Δ U = q + w$ . In special cases the statement can be expressed in different ways. Which of the following is not a correct expression?

The change in internal energy of the methanol is

For the reaction $C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l)$ the difference between enthalpy change and internal energy change is:

More topics

Internal Energy as a State of System

Overview

Learn

Videos

Study Materials

Quick summary with Stories

Heat as Internal Energy

First Law of Thermodynamics

Revise with Concepts

First Law of Thermodynamics

Internal Energy

Related questions

For which of the following reaction △H=△E+2RT

Assertion (A) : Zeroth law of thermodynamics gives us the concept of energy Reason (R) : Internal energy is dependent on temperature

One gram of water on evaporation at atmospheric pressure forms 1671 cm3 of steam. The heat of vaporisation at this pressure is 540 cal/gm. The increase in internal energy is

Energy hidden in a definite quantity of substance is:

The reaction between ΔG and ΔH is:

Which of the following statements are correct as per IUPAC sign convention?

According to the first law of thermodynamics, ΔU=q+w. In special cases the statement can be expressed in different ways. Which of the following is not a correct expression?

The change in internal energy of the methanol is

For the reaction C2​H4​(g)+3O2​(g)→2CO2​(g)+2H2​O(l) the difference between enthalpy change and internal energy change is:

Assuming that water vapour is an ideal gas, the internal energy change (ΔU) when 1mol of water is vapourised at 1bar pressure and 100∘C. (Given: Molar enthalpy of vapourisation of water at 1bar and 373K=41kJmol−1 and R=8.3Jmol−1K−1 will be )

More topics

For which of the following reaction $△ H = △ E + 2 R T$

Assertion (A) : Zeroth law of thermodynamics gives us the concept of energy
Reason (R) : Internal energy is dependent on temperature

One gram of water on evaporation at atmospheric pressure forms $1671 c m^{3}$ of steam. The heat of vaporisation at this pressure is $540 c a l / g m$ . The increase in internal energy is

The reaction between $Δ G$ and $Δ H$ is:

According to the first law of thermodynamics, $Δ U = q + w$ . In special cases the statement can be expressed in different ways. Which of the following is not a correct expression?

For the reaction $C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l)$ the difference between enthalpy change and internal energy change is: