Home
Class 11
CHEMISTRY
Given C(2)H(2)(g)+H(2)(g)rarrC(2)H(4)(g)...

Given `C_(2)H_(2)(g)+H_(2)(g)rarrC_(2)H_(4)(g): DeltaH^(@)=-175 " kJ mol"^(-1)`
`DeltaH_(f(C_(2)H_(4),g))^(@)=50 " kJ mol"^(-1), DeltaH_(f(H_(2)O,l))^(@)=-280 " kJ mol"^(-1), DeltaH_(f(CO_(2)g))^(@)=-390 " kJ mol"^(-1)`
If `DeltaH^(@)` is enthalpy of combustion (in kJ `"mol"^(-1)`) of `C_(2)H_(2)`(g), then calculate the value of `|(DeltaH^(@))/(257)|`

Text Solution

Verified by Experts

The correct Answer is:
5
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

From the following data CH_(3)OH(l)+(3)/(2)O_(2)(g) rarr CO_(2)(g) +2H_(2)O(l) Delta_(r) H^(@)=-726 kJ mol^(-1) H_(2)(g)+(1)/(2)O_(2)(g) rarr H_(2)O(l), Delta _(r) H^(@)=-286 kJ mol^(-1) C("graphite") +O_(2)(g) rarr CO_(2)(g), Delta _(r) H^(@)=-393 kJ mol^(-1) The standard enthalpy of formation of CH_(3)OH(l)" in "kJ mol^(-1) is

H_(2(g)) rarr 2H_((g)) , DeltaH = 400 KJ , then DeltaS_("system") at 2000 K is

2H_(2(g)) + O_(2(g)) rarr 2H_(2)O_((l)) , DeltaH= -ve and DeltaG= -ve . Then the reaction is

Calculate the enthalpy change for the process "CC"l_(4)(g)toC(g)+4CI(g) and calculate bond enthalpy of C-Cl in C Cl_(4)(g). Delta_("vap")H^(theta)("C C"l_(4))=30.5 kJ mol^(-1) . Delta_(f)H^(theta)(CCl_(4))=-135.5 kJ mol^(-1) . Delta_(0)H^(theta)(C)=715.0 kJ mol^(-1) , where Delta_(a)H^(theta) is enthalpy of atomisation. Delta_(a)H^(theta)(Cl_(2))=242 kJ mol^(-1) .

For the reaction 2H_(2(g)) + o_(2(g)) rarr 2H_(2)O_((g)), Delta H^(@) = - 573.2 kJ . The heat of decomposition of water per mol is:

If DeltaH_(f)^(0) " for" H_(2)O_(2(l)) and H_(2)O_((l)) " are " -188 kJ mol^(-1) and -286 kJ mol^(-1) , what will be the enthalpy change of the reaction 2H_(2)O_(2(l)) rarr 2H_(2)O_((l)) + O_(2(g)) = ?

The enthalpy changes for the following processes are listed below: Cl_(2(g)) rarr 2Cl_((g)) , DeltaH = 242.3 kJ mol^(-1) I_(2(g)) rarrr 2I_((g)) , DeltaH = 151.0 kJ mol^(-1) ICl_((g)) rarr I_((g)) + Cl_((g)) , DeltaH = 211.3 kJ mol^(-1) I_(2(s)) rarr I_(2(g)) , DeltaH = 62.76 kJ mol^(-1) Given that the standard states for iodine and chlorine are I_(2(s)) and Cl_(2(g)) , the standard enthalpy of formation for ICT is: