Most of the naturally occuring processes are spontaneous.
Find the temperature above which the reaction, `MgO(s) + C(s) rarr Mg(s) + CO(g)` becomes spontaneous. (Given `Delta_rH^@ = 490 kJ//mol` and `Delta_rS^@ = 198 J//molK`)

Most of the naturally occurring processes are spontaneous. a) Give the criteria for spontaneity of a process in terms of free energy change ( DeltaG ) b) Exothermic reactions associated with a decrease in entropy are sponaneous at lower temperatures. Justify on the basis of Gibbs equation. c) Find the temperature above which the reactin MgO_((s))+C_((s))rightarrow Mg_((s))+CO_((g)) becomes spontaneous. (Given ( Delta_rH^theta=490kJmol^-1 & Delta_rS^theta=198JK mol^-1 )

Given the following data: Determine at what temperature the following reaction is spontaneous? Fe O (s) + C (Graphite) to Fe (s) + CO (g)

The plot shows the variation of - In K_p versus temperature for the two reactions. M(s) + (1)/(2) O_2 (g) rarr MO (s) and C(s)+ (1)/(2) O_2(g) rarr CO(s) Identify the correct statement ,

For the reaction 2A+B rarr C at 298 K, DeltaH=400kJ mol^-1 and DeltaS=0.2 kJk^-1mol^_1 . At what temperature will be reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range.