3(6 points)Add dropwise a solution of Na2SO4 into a mixture of 0.010mol-LBa(NO)2 and 0.010mol-LCa(NO3)2.(1)predict via calculation which cation is precipitated first.(2)what the concentration of the first precipitated cation is when the second cation begins to precipitate?(K(CaS04)-9.1×10-6,K绵(BaS04F1.8x10-10) 4(9 points)Areaction 2HC+02(g)=Cl2(g)+H2O(g)will occur if you mix 0.080 mol air (volume fraction of O2 is20%,the rest is N2)with 0.020 mol HCI under 600K100.0kPa If volume fraction of Cl at equilibrium is 40%,calculate the reaction equilibrium constant Kand the partial pressure of N2. 5、(6 points)It is known that△fH2(C0,g=-110.5 kJ-mol，△fH%Ni(CO4,lF-605.0 kJ-mol S(Ni.s)=29.9J-molL.K-1,(CO.g)=197.9kJ-mor1.K,(Ni(CO).)=420.0kJ-mor1.K-1 calculate the temperature when Ni(CO)can be prepared,what the temperature is to decompose Ni(CO)forming pure Ni? 第6页3、(6 points) Add dropwise a solution of Na2SO4 into a mixture of 0.010mol·L-1Ba(NO)2 and 0.010mol·L-1Ca(NO3)2. (1) predict via calculation which cation is precipitated first; (2) what the concentration of the first precipitated cation is when the second cation begins to precipitate? (K (CaSO4)=9.1×10-6，K (BaSO4)=1.8×10-10) 4、(9 points) A reaction 2HCl+ 1 2 O2(g) Cl2(g)+H2O(g) will occur if you mix 0.080 mol air (volume fraction of O2 is 20%, the rest is N2) with 0.020 mol HCl under 600K、100.0kPa. If volume fraction of Cl2 at equilibrium is 40%, calculate the reaction equilibrium constant K and the partial pressure of N2. 5、(6 points) It is known that △fH (CO,g)=-110.5kJ·mol-1，△fH (Ni(CO)4,l)=-605.0kJ·mol-1， S (Ni,s)=29.9J·mol-1·K-1 ， S (CO,g)=197.9kJ·mol-1·K-1 ， S (Ni(CO)4,l)=420.0kJ·mol-1·K-1. calculate the temperature when Ni(CO)4 can be prepared, what the temperature is to decompose Ni(CO)4 forming pure Ni? 第 6 页