`CaCO_(3(s))rarr CaO_((s))+CO_(2(g))Delta H=+180kJ`. If entropies of limestone, lime and carbon dioxide are `93`, `39` and `213J/(mol.K)`. Then `Delta S_(t otal)` in `JK^(-1)` at `300K` is

For CaCO_(3)(s)rarr CaO(s)+CO_(2)(g) at 977^(@)C, Delta H = 174 KJ/mol , then Delta E is :-

For the reaction CaCO_(3(s)) hArr CaO_((s))+CO_(2(g))k_p is equal to

For CaCO_(3)(s) hArr CaO(s)+CO_(2)(g), K_(c) is equal to …………..

For CaCO_(3)(S) hArr CaO(s) + CO_(2) (g), Delta H = + Q at equilibrium. The addition of more CaCO3(s) causes?

K_(p) = 1, For the equilibrium CaCO_(3(s)) hArr CaO_((s)) + CO_(2(g)) . The temperature of the reaction can be given as :

The following are some state ments regarding dissociation of lime stone according to the equation CaCO_(3(s)) hArr CaO_((s)) + CO_(2(g)) : Delta H = 110 kJ. The reaction is carried in a closed vessel. A) The pressure of CO_(2) increases when temperature is inereased. B) The pressure of CO_(2) inereases when temperature is deereased C) The pressure of CO_(2) increases when amount of CaCO_(3) is decreased. The incorrect statements are .

For the reaction, CaCO_(3)(s) rarr CaO(s)+CO_(2)(g) , which is the correct representation?

Quick lime: (CaO) is produced bu heating limestone (CaCO_(3)) to derive off CO_(2) gas. CaCO_(3) (s) rarr CaO(s) +CO_(2)(g), Delta_(r)H^(Theta) = 180 k J mol^(-1), Delta_(r)S^(Theta) = 150 J K^(-1) Assuming that variation fo enthalpy change and entropy change with temperature to be negligible, which of the following is correct?

In a chemical reaction, Delta H = 150 kJ and Delta S = 100 JK^(-1) at 300 K. Therefore, Delta G will be

It is planned to carry out the reaction: CaCO_(3)(s) hArr CaO(s) +CO_(2)(g) at 1273K and 1 bar pressure. Delta_(r)G^(Theta) = 176 kJ mol^(-1) and Delta_(r)S^(Theta) = 157.2 kJ mol^(-1) a. Is the reaction spontaneous at this temperature and pressure ? b. Calculate the value of i. K_(p) at 1273K for the reaction ii. partial pressure of CO_(2) at equilibrium