The molar entropies of `HI_((g)), H_((g)) and I_((g))` at 298K are 206.5, 114.6, and `180.7 J mol^(-1)K^(-1)` respectively. Using the `DeltaG^(@)` given below, calculate the bond energy of HI. `HI_((g)) rarr H_((g)) + I_((g)), DeltaG^(@) = 271.8kJ` (Give your answer after divide with 49.7)
Given Delta H_r ^@ for CO_2(g) , CO_(g) and H_2O(g) are -393.5, -110.5 and -241.8 KJ mol^-1 respectively. The Delta H_r^@ (in KJ mol^-1] for the reaction CO_2(g) + H_2(g) rightarrow CO_(g) + H_2O(g) is
If DeltaG^@ for the reaction given below is 1. kJ, the equilibrium constant for a reaction. 2HI_((g)) harr H_(2(g))+I_(2(g)) at 25^@C is :
If the bond energies of H-H, Br-Br and HBr are 433, 192 and 364 kJ mol^(-1) respectively, then DeltaH^@ for the reaction : H_(2(g)) + Br_(2(g)) rarr 2HBr_((g)) is
If values of DeltaH_f^@ of ICl_((g)), Cl_((g)) and I_((g)) are respectively 17.57, 121.34, 106.96 J mol^(-1) . The value of I - Cl (bond energy) in J mol^(-1) is:
Standard entropies of H_(2)(g),O_(2)(g) " and "H_(2)O(l) are respectively 126.6, 201.2 and 68JK^(-1)mol^(-1) Determine DeltaS" for "2H_(2)(g)+O_(2)(g) to 2H_(2)O(l) at 25^(@)C .
At 298K heats of formation of H_(2)O_((l)), CO_(2(g)), HCl_((g)) and C Cl_(4(l)) are respectively -241.8, -393.7, -92.5 and -106.7 kJ mol^(-1) . Calculate DeltaH for the following reaction C Cl_(4(l)) + 2H_2O_((g)) to CO_(2(g)) + 4HCl_((g))
Estimate the average S-F bond energy in SF_(6) . The value of standard enthalpy of formation of SF_(6(g)), S_((g)) and F_((g)) " are" -1100, 275 and 80 kJ mol^ (-1) respectively. (Give your answer after divide with 51.5)
H_(2(g)) reacts with I_(2(g)) to give HI_((g)) . Write the rate equation and predict order.
NARENDRA AWASTHI-THERMODYNAMICS-Level 1 (Q.91 To Q.120)
