Home
Class 11
CHEMISTRY
Consider the following reaction betwee...

Consider the following reaction between zinc and oxygen and choose the correct options out of the options given below
`2Zn(s)+ O_(2)(g) to 2 ZnO_(s): DeltaH=-693.8 kJ mol^(-1)`

A

The enthalpy of two molesof ZnO is less than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8kJ

B

The enthalpy of two enthalpy of two moles of ZnO is more than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 Kj

C

693.8 kJ `mol^(-1)` energy is evolved in the reaction

D

`693.8 kJ mol^(-1)` energy is absorbed in the reaction.

Text Solution

Verified by Experts

The correct Answer is:
a,c
`DeltaH = H_(p) -H_(R)` . A negative value of `DeltaH ` shows that `H_(r) gt H _(p) `or `H_(p)lt H_(R)` , i.e.,enthalpy of two moles of ZnO is less than the enthalpy of two moles of zinc and one moleof oxygen by 693.8kJ , As `H_(R) gt H_(P)`, 693.8 kJ mol^(-1)` of energy is evolved in the reaction.
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    PRADEEP|Exercise NCERT EXEMPLAR PROBLEMS WITH ANSWERS, HINTS AND SOLUTIONS( SHORT ANSWER QUESTIONS)|31 Videos

  • THERMODYNAMICS

    PRADEEP|Exercise MATCHING TYPE QUESTIONS|8 Videos

  • THERMODYNAMICS

    PRADEEP|Exercise NCERT EXEMPLAR PROBLEMS WITH ANSWERS, HINTS AND SOLUTIONS( MULTIPLE CHOICE QUESTIONS-I)|14 Videos

  • STRUCTURE OF ATOM

    PRADEEP|Exercise Competition Focus (JEE (Main and Advanced)/Medical Entrance (IX. Assertion And Reason Type Questions (Type II))|12 Videos

Similar Questions

Explore conceptually related problems

For the following reaction, the value of K change with N_(2)(g)+O_(2)(g) lt lt 2NO(g), DeltaH=+180 kJ mol^(-1)

Assume DeltaH^(@) and DeltaS^(@) to be independent of temperature, at what temperature with the reaction given below becomes spontaneous? N_(2)(g) + O_(2)(g) to 2NO(g) DeltaH^(@) = 180.8 kJ mol^(-1)

Consider the following reactions. DeltaH^(@) values of the reactions hve been given as -x, -y and z kJ. Fe_(3)O_(4)(s) to 3Fe(s) + 2O_(2)(g), DeltaH^(@) = z kJ 2Fe(s) + O_(2)(g) to 2FeO(s), DeltaH^(@) =-x kJ 4Fe(s) + 3O_(2)(g) to 2Fe_(2)O_(3)(s), DeltaH^(@) =-y kJ In the given set of reaction, -x//2 kJ refers to

Consider the following reactions. DeltaH^(@) values of the reactions hve been given as -x, -y and z kJ. Fe_(3)O_(4)(s) to 3Fe(s) + 2O_(2)(g), DeltaH^(@) = z kJ 2Fe(s) + O_(2)(g) to 2FeO(s), DeltaH^(@) =-x kJ 4Fe(s) + 3O_(2)(g) to 2Fe_(2)O_(3)(s), DeltaH^(@) =-y kJ Heat of reaction for the reaction, FeO(s) + Fe_(2)O_(3)(s) to Fe_(3)O_(4)(s) is :

Calculate the standard enthalpy of formation of SO_3 at 298 K using the following reactions and enthalpies. S_(8)(s) + 8O_2(g) to 8SO_2(g), DeltaH^(@) = -2775 kJ mol^(-1) 2SO_(2)(g) + O_(2)(g) to 2SO_(3)(g), Delta H^(@) = - 198 kJ mol^(-1) .

The factor of DeltaG values is important in metallurgy. The DeltaG values for the following reactions at 800°C are given as : S_(2)(s) + 2O_(2)(g) to 2SO_(2)(g), DeltaG =-544 kJ 2Zn(s) + S_(2)(s) to 2ZnS(s), DeltaG=-293 kJ 2Zn(s) + O_(2)(g) to 2ZnO(s), DeltaG = -480 kJ Calculate the DeltaG for the reaction: 2ZnS(s) + 3O_(2)(g) to 2ZnO(s) + 2SO_(2)(g)

Diborane is a potentail rocket fuel which undergoes combusion according to the reaction B_(2)H_(6)(g)+3O_(2)(g)rarrB_(2)O_(3)(s)+3H_(2)O(g) From the following data, calculate the enthalpy change for the combustion of diborane 2B(s)+(3//2)O_(2)(g)rarrB_(2)O_(3)(s) DeltaH= -1273 kJ mol^(-1) H_(2)(g)+(1//2)O_(2)(g)rarrH_(2)O(1) " "Delta H= -286 kJ mol^(-1) H_(2)O(1)rarrH_(2)O(g)" "DeltaH=44 kJ mol^(-1) 2B(s)+3H_(2)(g)rarrB_(2)H_(6)(g)" "Delta H= 36kJ mol^(-1)