Consider the following reaction between zinc and oxygen and choose the correct options out of the options given below
2 Zn(s)+O2(g)→2 ZnO(s);ΔH=−693.8 kJ mol−1
(a) The enthalpy of two moles of ZnO is less than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ
(b) The 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
Consider the following reaction between zinc and oxygen and choose the correct options out of the options given below
2 Zn(s)+O2(g)→2 ZnO(s);ΔH=−693.8 kJ mol−1
(a) The enthalpy of two moles of ZnO is less than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ
(b) The 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
For the reaction,
2 Zn(s)+O2(g)→2 ZnO(s);ΔH=−693.8 kJ mol−1
As we know that, ΔH=HP=HR
A negative value of ΔH shows that HR>HP or HP<HR i.e., enthalpy of two moles of ZnO is less than the enthalpy of two moles of zinc and one mole of oxygen by 693.8kJ. As HR>HP 693.8kJ mol−1'of energy is evolved in the reaction.(c)
For the reaction,
2 Zn(s)+O2(g)→2 ZnO(s);ΔH=−693.8 kJ mol−1
As we know that, ΔH=HP=HR
A negative value of ΔH shows that HR>HP or HP<HR i.e., enthalpy of two moles of ZnO is less than the enthalpy of two moles of zinc and one mole of oxygen by 693.8kJ. As HR>HP 693.8kJ mol−1'of energy is evolved in the reaction.(c)
