At 300 K, the reactions which have following values of thermodynamic parameters occur spontaneouslyA. `DeltaG^(@)=-400 kJ mol^(-1)`B. `DeltaH^(@)=200 kJ mol^(-1), DeltaS^(@)=-4 JK^(-1) mol^(-1)`C. `DeltaH^(@)=-200 kJ mol^(-1), DeltaS^(@)=4 JK^(-1) mol^(-1)`D. `DeltaH^(@)=200 J mol^(-1), DeltaS^(@)=40 JK^(-1)mol^(-1)`

At 300 K, the reactions which have following values of thermodynamic p

1.	At 300 K, the reactions which have following values of thermodynamic parameters occur spontaneouslyA. `DeltaG^(@)=-400 kJ mol^(-1)`B. `DeltaH^(@)=200 kJ mol^(-1), DeltaS^(@)=-4 JK^(-1) mol^(-1)`C. `DeltaH^(@)=-200 kJ mol^(-1), DeltaS^(@)=4 JK^(-1) mol^(-1)`D. `DeltaH^(@)=200 J mol^(-1), DeltaS^(@)=40 JK^(-1)mol^(-1)`
Answer» Correct Answer - A::C::D When `DeltaH=+ve` and `DeltaS=-ve` than the reaction is non-spontaneous.

Discussion

No Comment Found

Related InterviewSolutions

Which of the following statement is true. The entropy of the universeA. Increases and tends towars maximum valueB. Decreases and tends to be zeroC. Remains constantD. Decreases and increases with a periodic rate
For the homogenous reaction `xA+yB iff 1Y + mZ DeltaH^(@) = -30kJ mol^(-1) and DeltaS=-100JK mol^(-1)` At what temperature the reaction is at equilibriumA. `50^(@)C`B. `250^(@)C`C. 100 KD. `27^(@)C`
The enthalpy change for the reaction `C_(2)H_(2)(g)+(5)/(2)O_(2)rarr2CO_(2)(g)+H_(2)O(g)` is known as enthalpy ofA. FormationB. FusionC. VaporizationD. Combustion
The free energy change for the following reactions are given below, `C_(2)H_(2)(g)+(5)/(2)O_(2)(g)rarr2CO_(2)(g)+H_(2)O(l),DeltaG^(@)=-1234 kJ` `C(s)+O_(2)(g)rarrCO_(2)(g)DeltaG^(@)=-394 kJ` `H_(2)(g)+(1)/(2)O_(2)(g)rarrH_(2)O(l)DeltaG^(@)=-237 kJ` What is the standard free energy change for the reaction `H_(2)(g)+2C(s)rarrC_(2)H_(2)(g)`A. `-209 kJ`B. `-2259 kJ`C. `+2259 kJ`D. 209 kJ
When 100 mL of 1.0 M HCl was mixed 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase `5.7^(@)C` was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant `(-57.0 kJmol^(-1))`, this experiment could be used to measure the calorimeter constant. In a second experiment (Expt.2) 100 mL of 2.0 M acetic acid `(K_(a)=2.0xx10^(-5))` was mixed with 100 mL of 1.0 M NaOH (under indentical conditions to Expt. 1) where a temperature rise of `5.6^(@)C` was measured (Consider heat capacity of all solutions as `4.2 Jg^(-1)K^(-1)` and density of al solutions as 1.0 gm`L^(-1)`) The pH of the solution after Expt. 2 isA. `2.8`B. `4.7`C. `5.0`D. `7.0`
When 100 mL of 1.0 M HCl was mixed 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase `5.7^(@)C` was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant `(-57.0 kJmol^(-1))`, this experiment could be used to measure the calorimeter constant. In a second experiment (Expt.2) 100 mL of 2.0 M acetic acid `(K_(a)=2.0xx10^(-5))` was mixed with 100 mL of 1.0 M NaOH (under indentical conditions to Expt. 1) where a temperature rise of `5.6^(@)C` was measured (Consider heat capacity of all solutions as `4.2 Jg^(-1)K^(-1)` and density of al solutions as 1.0 gm`L^(-1)`) Enthalpy of dissociation (in `KJmol^(-1)`) of acetic acid obtained from the Expt.2 isA. `1.0`B. `10.0`C. `24.5`D. `51.4`
In a constant volume calorimeter, 3.5g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K. The temperature of the calorimeter was found to increase from 298.0K to 298.45 K due to the combustion of the gas in kJ `mol^(-1)` is
The amount of heat evolved when `500cm^(3)` of 0.1M HCl is mixed with `200cm^(3)` of 0.2 M NaOH isA. 2.292 kJB. 1.292 kJC. 0.292 kJD. 3.392 kJ
In which of the following reactions, the heat liberated is known as 'heat of combustion'.A. `H_((aq))^(+)+OH_((aq))^(-)rarrH_(2)O_((l))+"heat"`B. `C("graphite")+(1)/(2)O_(2(g))rarrCO_((g))+"heat"`C. `CH_(4(g))+2O_(2(g))rarrCO_(2(g))+2H_(2)O_((l))+"heat"`D. `H_(2)SO_(4(aq))+H_(2)O_((l))rarrH_(2)SO_(4(aq))+"heat"`
When 0.5g of sulphur is burnt to `SO_(2), 4, 6 kJ of heat is liberated. What is the enthalpy of formation of sulphur dioxideA. `+ 147.2 kJ`B. `- 147.2 kJ`C. `- 294.4 kJ`D. `+ 294.4 kJ`

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment