Thermodynamics ...

Suppose that a reaction has $$\Delta H=-40kJ$$ and $$\Delta S=-50J/K$$. At what temperature range will it change from spontaneous to non-spontaneous ?

Consider the reaction, $$2A_{(g)} + B_(g) rightleftarrow 2C_{(g)}$$ for which $$K_c = 350$$. If $$0.01$$ mole of each of the reactants and product are mixed in a $$2.0$$L flask, then the reaction quotient and the spontaneous direction of the system will be?

$$\Delta H$$ and $$\Delta S$$ are $$-283\ kJ$$ and $$-87\ J\ K^{-1}$$, respectively. It was intended to carry out this reaction at $$1000, 1500, 3000$$ and $$3500\ K$$. At which of these temperatures would this reaction be thermodynamically spontaneous?

Which of the following statements is wrong?

Which of the following is not true about a reversible reaction?

$$2{H}_{2(g)}+{O}_{2(g)}\rightarrow 2{H}_{2}{O}_{(l)};\Delta H=-ve$$ and $$\Delta G=-ve$$. Then the reaction is

Which of the following expression for an irreversible process:

In standard state the non spontaneous reaction among the following is:

Answer the question based on the diagram involving $$1$$ mole of ideal gas.
Process $$A\rightarrow B$$ represents: