Home
Class 11
CHEMISTRY
Calculate the heat produced (in kJ) when...

Calculate the heat produced (in kJ) when 224 gm of CaO is completely converted to `CaCO_(3)` by reaction with `CO_(2)` at `27^(@)` in a container of fixed volume.
Given : `DeltaH_(f)^(@)(CaCO_(3),s)=-1207kJ//mol," "DeltaH_(f)^(@)(CaO,s)=-635kJ//mol`
`DeltaH_(f)^(@)(CO_(2),g)=-394kJ//mol,["Use R"=8.3JK^(-1)mol^(-1)]`

A

`702.04` kJ

B

`721.96` kJ

C

712 kJ

D

721 kJ

Text Solution

Verified by Experts

The correct Answer is:
A
`CaO(s)+CO_(2)(g)rarrCaCO_(3)(s)`
`Delta_(f)H^(@)=DeltaH_(f)^(@)(CaCO_(3))-DeltaH_(f)^(@)(CaO)-DeltaH_(f)^(@)(CO_(2))`
`=-1207 -(-635)-(-394)`
=-178 kJ/mol
`thereforeDeltaU=DeltaH-Deltan_(g)RT`
`DeltaU=-178-((-1)xx8.3 xx300)/(1000)`
=-175.51 kJ
`n_(CaO)=(224)/(56)=4`
`thereforeq_(v)=n.Delta_(r)U=4xx(-175.51)`
=-702.04 kJ
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    NARENDRA AWASTHI|Exercise Level 1 (Q.1 To Q.30)|6 Videos

  • THERMODYNAMICS

    NARENDRA AWASTHI|Exercise Level 1 (Q.31 To Q.60)|2 Videos

  • STOICHIOMETRY

    NARENDRA AWASTHI|Exercise Level 3 - Subjective Problems|20 Videos

Similar Questions

Explore conceptually related problems

For the following cell reaction, Ag | Ag^(+) | AgCl | Cl^(-) | Cl_(2) , Pt Delta G_(f)^(0) (AgCl) =-109 kJ//mol Delta G_(f)^(0) (Cl ) = -129kJ//mol Delta G_(f)^(0) (Ag^(+)) = 78 kJ//mol E^@ of the cell is

Calculate a) DeltaG^(@) and b) the equilibrium constant for the formation of NO_(2) from NO and O_(2) at 298K NO(g)+1//2O_(2)(g)hArrNO_(2)(g) where Delta_(f)G^(oplus)(NO_(2))=52.0kJ//mol Delta_(f)G^(oplus)(NO)=87.0kJ//mol Delta_(f)G^(oplus)(O_(2))=0kJ//mol

The bond dissociation energy depends upon the nature of the bond and nature of the molecule. If any molecule more than 1 bonds of similar nature are present then the bond energy reported is the average bond energy. Determine C-C and C-H bond enthalpy (in kJ/mol). Given: Delta_(f)H^(0) (C_(2)H_(6),g)= -85kJ//mol, Delta_(f) H^(0) (C_(3)H_(8), g)= -104kJ//mole, Delta_("sub")H^(0) (C,s)= 718kJ//mol , B.E. (H-H)= 436 kJ/mol,

What is the standard enthalpy of rection (in kJ) when two moles of Fe_(2)O_(3) (s) reacts with H_(2) gas to give Fe metal? DeltaH_(f)^(@) of Fe_(2)O_(3)(s)andH_(2)O(l) are -824.2 and -285.83kJmol^(-1) respectively.

DeltaH^(0) for a reaction F_(2) + 2HCl rarr 2HF + Cl_(2) is given as -352.8 kJ. Delta H_(f)^(0) for HF is -268.3 KJ mol^(-1) , then Delta H_(f)^(0) of HCl would be

Consider the following reaction : CO_((g)) + 2H_(2(g)) hArr CH_(3)OH_((g)) Given : Delta_(r) H^(@) (CH_(3)OOH, g) = -201 kJ/mol, Delta_(r) H^(@) (CO, g) = -114 kJ/mol S^(@) (CH_(3)OOH, g) = 240 J/K-mol , S^(@) (H_(2), g) = 29 JK^(-1)mol^(-1) S^(@) (CO, g) = 198 J/mol-K , C^(@)_(p,m) (H_(2)) = 28.8 J/mol-K C^(@)_(p,m) (CO) = 29.4 J/mol-K , C^(@)_(p,m) (CH_(3)OH) = 44 J/mol-K and ln ((320)/(300)) = 0.06 , all data at 300 K Delta_(r) S^(@) at 300 K for the reaction is :

Consider the following reaction : CO_((g)) + 2H_(2(g)) hArr CH_(3)OH_((g)) Given : Delta_(r) H^(@) (CH_(3)OH, g) = -201 kJ/mol, Delta_(r) H^(@) (CO, g) = -114 kJ/mol S^(@) (CH_(3)OOH, g) = 240 J/K-mol , S^(@) (H_(2), g) = 29 JK^(-1)mol^(-1) S^(@) (CO, g) = 198 J/mol-K , C^(@)_(p,m) (H_(2)) = 28.8 J/mol-K C^(@)_(p,m) (CO) = 29.4 J/mol-K , C^(@)_(p,m) (CH_(3)OH) = 44 J/mol-K and ln ((320)/(300)) = 0.06 , all data at 300 K Delta_(r) S^(@) at 320 K is :

Consider the following reaction : CO_((g)) + 2H_(2(g)) hArr CH_(3)OH_((g)) Given : Delta_(r) H^(@) (CH_(3)OOH, g) = -201 kJ/mol, Delta_(r) H^(@) (CO, g) = -114 kJ/mol S^(@) (CH_(3)OOH, g) = 240 J/K-mol , S^(@) (H_(2), g) = 29 JK^(-1)mol^(-1) S^(@) (CO, g) = 198 J/mol-K , C^(@)_(p,m) (H_(2)) = 28.8 J/mol-K C^(@)_(p,m) (CO) = 29.4 J/mol-K , C^(@)_(p,m) (CH_(3)OH) = 44 J/mol-K and ln ((320)/(300)) = 0.06 , all data at 300 K Delta_(r) H^(@) at 300 K for the reaction is :