हिंदी

Answer the following in one or two sentences. What is standard state of a substance?

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प्रश्न

Answer the following in one or two sentences.

What is standard state of a substance?

लघु उत्तरीय
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उत्तर

  1. The standard state of a substance is the form in which the substance is most stable at a pressure of 1 bar and at a temperature of 298 K.
  2. If the reaction involves species in solution, its standard state is 1 M concentration.
    e.g. Standard states of certain elements and compounds are (at 1 bar and 25 °C); \[\ce{H2_{(g)}, Hg_{(l)}, Na_{(s)}, C_{(graphite)}, C2H5OH_{(l)}, CaCO3_{(s)}, CO2_{(g)}, C2H5OH_{(l)}, H2O_{(l)}, CaCO3_{(s)}, CO2_{(g)}}\].
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अध्याय 4: Chemical Thermodynamics - Exercises [पृष्ठ ८७]

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बालभारती Chemistry [English] Standard 12 Maharashtra State Board
अध्याय 4 Chemical Thermodynamics
Exercises | Q 2.4 | पृष्ठ ८७

संबंधित प्रश्न

Answer the following question.

State Hess’s law of constant heat summation. Illustrate with an example. State its applications.


Answer the following question.

Calculate ΔrH° for the following reaction at 298 K:

1) 2H3BO3(aq) → B2O3(s) + 3H2O(l), ΔrH° = + 14.4 kJ

2) H3BO3(aq) → HBO2(aq) + H2O(l), ΔrH° = - 0.02 kJ

3) H2B4O7(s) → 2B2O3(s) + H2O(l), ΔrH° = + 17.3 kJ


The enthalpy change of the following reaction:

\[\ce{CH_{4(g)} + Cl_{2(g)} -> CH3Cl_{(g)} + HCl_{(g)}ΔH^0 = –104 kJ}\]

Calculate C – Cl bond enthalpy. The bond enthalpies are:

Bond C − H Cl − Cl H − Cl
∆H°/kJ mol−1 414 243 431

Define standard enthalpy of formation.


Write an application of Hess’s law.


Classify the following into intensive and extensive properties.

Pressure, volume, mass, temperature.


When 6.0 g of graphite reacts with dihydrogen to give methane gas, 37.4 kJ of heat is liberated. What is standard enthalpy of formation of CH4 (g)?


The heat of formations of CO(g) and CO2(g) are −26.4 kcal and −94.0 kcal respectively. The heat of combustion of carbon monoxide will be ____________.


The standard heats of formation in kcal mol−1 of NO2(g) and N2O4(g) are 8.0 and 2.0 respectively. The heat of dimerization of NO2 in kcal is ____________.

\[\ce{2NO2_{(g)} ⇌ N2O4_{(g)}}\]


The enthalpy change accompanying a reaction in which 1 mole of the substance in the standard state reacts completely with oxygen or is completely burnt is called as ____________.


lf, \[\ce{C_{(s)} + O2_{(g)} -> CO2_{(g)}}\], ∆H = x .........(i)

\[\ce{CO_{(g)} + 1/2O2_{(g)} -> CO2_{(g)}}\], ∆H = y .......(ii)

Then, the heat of formation of CO is:


\[\ce{S + 3/2O2 -> SO3 +2{x} kcal}\] .........(i)

\[\ce{SO2 + 1/2O2 -> SO3 + {y} kcal}\] .......(ii)

The heat of formation of SO2 is ____________.


Which among the following salts, solubility decreases with increase in temperature?


Calculate the enthalpy of hydrogenation of C2H4(g), given that the enthalpy of formation of ethane and ethylene are −30.2 kcal and +12.5 kcal respectively.


Standard enthalpy of formation of water is - 286 kJ mol-1. When 1800 mg of water is formed from its constituent elements in their standard states the amount of energy liberated is ______.


Which of the following equations has ΔfH° and ΔH° same?


Calculate the standard enthalpy of:

\[\ce{N2H_{4(g)} + H_{2(g)} -> 2NH_{3(g)}}\]

If ΔH0(N – H) = 389 kJ mol–1, ΔH0(H – H) = 435 kJ mol–1, ΔH0(N – N) = 159 kJ mol–1.


Identify the invalid equation.


What is the amount of water formed by the combustion of 1.6 g methane?


Calculate the standard enthalpy of the reaction, \[\ce{SiO2_{(s)} + 3C_{(graphite)} -> SiC_{(s)} + 2CO_{(g)}}\] from the following reactions:

  1. \[\ce{Si_{(s)} + O2_{(g)} -> SiO2_{(s)}}\], ΔrH0 = −911 kJ
  2. \[\ce{2C_{(graphite)} + O2_{(g)} -> 2CO_{(g)}}\], ΔrH= −221 kJ
  3. \[\ce{Si_{(s)} + C_{(graphite)} -> SiC_{(s)}}\], ΔrH= −65.3 kJ

For the reaction, aA + bB → cC + dD, write the expression for enthalpy change of reaction in terms of enthalpies of formation of reactants and products.


The enthalpy of combustion of S (rhombic) is − 297 kJ mo1-1. Calculate the amount of sulphur required to produce 29. 74 kJ of heat.


The heat evolved in the combustion of 6.022 x 1021 carbon particles is 3.94 kJ. The heat of combustion of carbon is ______.


For the reaction, H2 + I2 ⇌ 2HI; ΔH = 12.4 kcal. The heat of formation of HI, ΔHf = ______.


Calculate heat evolved for combustion of 13 gm of acetylene (C2H2).

Given: \[\ce{C2H2_{(g)} + 5/2O_{2(g)}-> 2CO_{2(g)} + H2O_{(l)} \Delta_{(c)}H^{0} = - 1300 kJ}\]


Calculate the standard enthalpy of combustion of methane if the standard enthalpy of formation of methane, carbon dioxide and water are −74.8, −393.5 and −285.8 kJmol−1 respectively.


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