The standard reaction Gibbs energy for a temperature T is given by `Delta_(r)G^(@)= A-Bt` Where A and B are non-zero constants. Which of the following is TRUE about this reaction ?
The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given by Delta_(r)G^(0)=A-BT where A and B are non-zero constant.Which of the following is true about this reaction? (A) Exothermic if "A>0" and "B 0" (C) Exothermic if "A>0" (D) Endothermic if "B<0"
Which of the following statements about zero order reaction is not true
For the chemical reaction X Y , the standard reaction Gibbs energy depends on temperature T (in K) as Delta_rG^0 ( in kJ mol^(-1) ) = 120-3/8 T . The major component of the reaction mixture at T is
A reaction is spontaneous at low temperature but non- spontaneous at high temperature. Which of the following is true for the reaction?
Thermal decomposition of gaseous X_(2) to gaseous X at 298K takes place according to the following equation: X(g)hArr2X(g) The standard reaction Gibbs energy Delta_(r)G^(@) , of this reaction is positive. At the start of the reaction, there is one mole of X_(2) and no X . As the reaction proceeds, the number of moles of X formed is given by beta . Thus beta_("equilibrium") is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. [Given, R=0.083L bar K^(-1) mol^(-1) ) The incorrect statement among the following for this reaction, is
If an endothermic reaction occurs spontaneously at constant T and P , then which of the following is true
