In which of the following reactions will a change in pressure not affect the rate of reaction?

According to Le $Chatelier$ principle,if heat is given to a solid-liquid system,then:

For the reaction $SO_{2(g)} + 1/2 O_{2(g)} \rightleftharpoons SO_{3(g)}$,the percentage yield of product at different pressures is shown in the figure. Then,which among the following is true?

Consider the following reactions. In which cases is product formation favoured by decreased temperature?
$(a) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}; \ \Delta H^o = 181 \ kJ$
$(b) \ 2CO_{2(g)} \rightleftharpoons 2CO_{(g)} + O_{2(g)}; \ \Delta H^o = 566 \ kJ$
$(c) \ H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}; \ \Delta H^o = -9.4 \ kJ$
$(d) \ H_{2(g)} + F_{2(g)} \rightleftharpoons 2HF_{(g)}; \ \Delta H^o = -541 \ kJ$

What is the effect of adding $Kr$ (krypton) gas at equilibrium while keeping the volume of the system constant?

$KMnO_4$ can be prepared from $K_2MnO_4$ as per the reaction:
$3MnO_4^{2-} + 2H_2O \rightleftharpoons 2MnO_4^- + MnO_2 + 4OH^-$
The reaction can go to completion by removing $OH^-$ ions by adding: