At 298K, the equilibrium constant for the following reaction is 4.20x10-7: H2CO3(aq) + H2O= H30*(aq) + HCO3"(aq) The equilibrium constant for a second reaction is 4.80x10-11: HCO3 (aq) + H20= H30*(aq) + CO32-(aq) Use this information to determine the equilibrium constant for the reaction: H2CO3(aq) + 2H20= 2H30*(aq) + CO32-(aq) K =

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A: H2(g) + I2(s) ----> 2HI (g) Mass of iodine = 25.6 g Molar mass of I2 = 253.80 g/mol  

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Q: solution? 3. What is the molarity of 500-mL solution which contains 40 g urea (CH«N2O)?

A: Given-> Volume = 500 ml = 0.500 L (1 L = 1000 ml) Weight of urea = 40 gm Molarity =?    

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A: Given: Concentration of hydroxide i.e. OH- ions, [OH- ] = 0.0137 M  

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Q: öf barium phosphate that will dissolve in a 0.103 M barium nitrate solution is M. Submit Answer Retr...

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A: Given : We have to calculate the mass of Mg.

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Q: Spektra C 80 40 20 4000 3500 3000 2500 2000 1500 1000 500 FLOCHEH OCUO

A: There are a few easily recognizable peaks in the spectra as discussed in the following step. 

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Q: Br2(g) + OCl2(9)- BrOC1(g) + BrCl(g) Kp is equal to 54.45. A reaction vessel is filled with 2.6 atm ...

A: ★ Answer : Equilibrium pressure of BrOCl will be 2.29 atm. ★ Solution : 

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Q: ... Page 15 of 16 CHEMISTRY2400 EXPERIMENT 8: PRIMARY HALOALKANE: NUCLEOPHILIC SUBSTITUTION WINTER 2...

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A: The solution is given below - 

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A: Given- ∆H°f(H2O)=-285.8kJ/mol ∆H°f(CO2)=-393.5kJ /mol ∆H°f(O2)=0kJ/mol    

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Q: Solid potassium chromate is slowly added to 50.0 mL of a calcium nitrite solution until the concentr...

A: Given: Concentration of CrO42- = 0.0247 M  

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Q: er of molecules in excess is

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A: The sentence is true. 

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Q: Fill in the missing chemical formulae in the tables below. acid conjugate base H,0 ? H,PO4 H,O"

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A: mass of magnesium nitride =  12.0 grams mass of water = 17.5 grams

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