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`