1)One of the sodium oxoacid salts of chlorine was analyzed. A 17.00 g sample was found to contain 3.68 g Na and 5.67 g Cl. The empirical formula of...
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1)One of the sodium oxoacid salts of chlorine was analyzed. A 17.00

g sample was found to contain 3.68 g Na and 5.67 g Cl. The empirical formula of this salt is
A. Na2Cl3O4
B. NaClO2
C. NaClO3
D. NaClO
E. Na2Cl2O3


2)The reaction between silver nitrate (AgNO3) and barium chloride (BaCl2), both dissolved in aqueous solution, yields a precipitate of silver chloride (AgCl) and a solution containing barium nitrate [Ba(NO3)2]. One way to balance this reaction is
2 AgNO3 + BaCl2 → 2 AgCl + Ba(NO3)2
 
A second way to balance this reaction is
2 AgNO3 + BaCl2 → Ag2Cl2 + Ba(NO3)2
 
This second method is


A. correct
B. not correct
C. correct, but only when excess AgNO3 is used
D. correct, but only when excess BaCl2 is used


3)For the equation
w Fe2S3 + y O2→ x Fe2O3 + z SO2 to be properly balanced, the values of w, y, x and z must be
A. 2, 7, 2 and 6
B. 2, 9, 2 and 6
C. 1, 9, 1 and 3
D. all coefficients are equal to 1


4)Consider the reaction below:
Al4C3 + 12 H2O → 3 CH4 + 4 Al(OH)3.
The yield of Al(OH)3 from 6.0 mol of water is:


A. 3.0 mol
B. 2.0 mol
C. 0.50 mol
D. 3.0 mol
E. 6.0 mol


5)For the balanced reaction
4 NH3 + 3 O2 →2 N2 + 6 H2O
(Atomic masses: H = 1.0 g/mol; N = 14.0 g/mol; O = 16.0 g/mol), the mass of ammonia needed to react with 106 g of O2 is


A. 141 g
B. 75 g
C. 188 g
D. 53 g
E. 106 g

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