3 mole of Ag is heated from 300K to 1000K calculate `triangleH` when `P=1` atm and `C_(p)=23+0.01T`

For silver, C_(P)(J K^(-1)"mol"^(-1))=23+0.01T . If the temperature (T) of 3 moles of silver is raised from 300K to 1000K at 1 atm pressure, the value of DeltaH will be close to :

For silver, C_p(JK^(-1)mol^(-1))=23+0.01T If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of 'Delta H' will be close to

For an element, Cp = 23 + 0.01 T("JK"^(-1)"mol"^(-1)) . If temperature of 3 moles of that element is raised from 300 K to 1000 K at 1 atm pressure, the value of DeltaH will be ______ kJ.

Molar heat capacity of an ideal gas at constant volume is given by C_(V)=2xx10^(-2)J (in Joule). If 3.5 mole of hits ideal gas are heated at constant volume from 300K to 400K the change in internal energy will be

10 moles of a gas are heated at constant volume from 20^@C" to "30^@C . Calculate the change in the internal energy of the gas. The molar heat capacity of the gas at constant pressure, C_p = 6.82 cal K^(-1) mol^(-1) and R = 1.987 cal K^(-1) mol^(-1) .

When two moles of an ideal gas (C_(p.m.)=(5)/(2)R) heated form 300K to 600K at constant pressure, the change in entropy of gas (DeltaS) is:

If liquefied oxygen at 1 atmospheric pressure is heated from 50K to 300k by supplying heat at constant rate. The graph of temperature vs time will be

Select the correct enthalpy at corresponding temperature using following datas (i) Heat capacity of solid from 0K to normal melting point 200K C_(p.m)(s)=0.035T" "JK^(-1)"mol"^(-1) (ii) Enthalpy of fusion =7.5 KJ"mol"^(-1) (iii) Enthalpy of vaporisation =30KJ "mol"^(-1) (iv) Heat capacity of liquid form 200K to normal boiling point 300K C_(p.m)(l)=60+0.016T " "JK^(-1)"mol"^(-1) (v) Heat capacity of gas from 300 K to 600 K at 1 atm C_(p.m)(g)=50.0" " JK^(-1)"mol"^(-1)

The molar internal energy of a gas over a temperature range is expressed as: U_(m) (T) =a +bT +cT^(2) , where b = 16 J mol^(-1)K^(-1) and c = 6 xx 10^(-3) J mol^(-1)K^(-2) . Find: a. C_(V,m)at 300K b. The entropy change when 1 mol of a gas is heated from 300K to 600K at constant volume.

For the reaction: CO(g) +H_(2)O(g) hArr CO_(2)(g) +H_(2)(g) (Delta_(r)H)_(300K) = - 41.2 kJ mol^(-1) (Delta_(r)H)_(1200K) =- 33.0 kJ mol^(-1) (Delta_(r)S)_(300K) = - 4.2 xx 10^(-2) kJ mol^(-1) (Delta_(r)S)_(1200K) =- 3.0 xx10^(-2) kJ mol^(-1) Predict the direction of spontaneity of the reaction at 300K and 1200K . also calculated log_(10)K_(p) at 300K and 1200K .