Asked by anirbanbag81 | 9th Jan, 2018, 10:34: AM
Option (3) is correct.
Answered by Varsha | 9th Jan, 2018, 12:05: PM
- write a relation between delta G and Q and define the meaning of each term and answer the following a) why a reaction proceeds forward when Q< K and no net reaction occurs when Q = K b) explain the effect of increase in pressure in terms of reaction quotient Q for the reaction CO ⇆ CH4(g) + H2O(g) (ii) for the reaction, N2(g) +3H2(g)⇆ 2NH(g) at 400K , Kp = 41, find the value Kp for the reaction 2N2(g) +6H2(g) ⇆ 4NH3(g)
- Give the relationship between Gibbs energy change and equilibrium constant?
- What is the relation between ?
- At what temperature the entropy of a perfectly crystalline substance is zero?
- For a reaction, Determine the temperature above which reaction will be spontaneous.
- Calculate the entropy of vaporization of water if its enthalpy of vaporization is 186.5 kJmol-1?
- For a water gas reaction at 1000°C the standard Gibb’s energy change is -8.1 kJ mol-1. Calculate the value of equilibrium constant?
- Calculate the standard Gibbs energy change for the following reaction: Given that for Cu2+(aq) and Zn2+(aq) as 65 kJ mol-1 and -147.2 kJ mol-1 respectively.
- For the reaction: Calculate the temperature at which Gibbs energy change ΔG is equal to zero. Predict the nature of the reaction at this temperature and above it.
- Calculate the standard energy Gibbs energy change for the formation of propane, C3H8 (g) at 298 K. Given that For propane = -103.85 kJmol-1S° mC3H8 (g) =270.2 JK-1 mol-1, S° m H2 (g) = 130.68 Jk-1mol-1 and S° m C(graphite) = 5.74 JK-1 mol-1
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