General Chemistry Answers

10.3 moles of H2O are produced. How

many moles of Fe are also produced?

A. 15.5 mol Fe

B. 6.87 mol

C. 5.2 mol Fe

D. 20.6 mol Fe

25.0 g H2 are reacted, how much Fe is

produced?

Molar masses: 2.02 g/mol H2, 55.9 g/mol Fe

A. 0.903 g Fe

B. 1,112 g Fe

C. 692 g Fe

D. 346 g Fe

If 0.425 mol H2O are produced, how

many moles of CO3 were reacted?

A. 0.425 mol CO3

B. 0.850 mol CO3

C. 0.213 mol CO3

D. 0.626 mol CO3

If 1.20 g CO3 are reacted, how much NH3

will be produced?

Molar masses:

60.0 g/mol CO3, 17.0 g/ mol NH3

A. 0.17 g CO3

B. 0.68 g CO3

C. 8.47 g CO3

D. 2.12 g CO3

If 0.425 mol HO are produced, how

many moles of CO3 were reacted?

A. 0.425 mol CO3

B. 0.850 mol CO3

C. 0.213 mol CO3

D. 0.626 mol CO3

25.0 g H, are reacted, how much Fe is

produced?

Molar masses: 2.02 %mol Ha, 55.9 %/mol Fe

A. 0.903 g Fe

B. 1,112 g Fe

C. 692 g Fe

D. 346 g Fe

10.3 moles of H,O are produced. How

many moles of Fe are also produced?

A. 15.5 mol Fe

B. 6.87 mol

C. 5.2 mol Fe

D. 20.6 mol Fe

If 17.3 g SO, are reacted, how much O

is consumed?

Molar masses: 32.0 %/mol O2, 64.0 9/mol SO2

A. 17.3 g 02

B. 0.135 g O

C. 0.270 g 0,

D. 4.33 g 02

What concentration results when 1.7 L of 0.45 mol/L Ba (OH)2 is mixed with 600 mL of 1.70 mol/L Ba(OH)2?

tritrations were performed on a 300.00mL samples of water taken from Lake Ontario. 4 trials were done. 54.5 mL/35.8 mL/ 53.8 mL/54.1 mL of 0.020 mol/L KOH was used to neutralize the sulphuric acid (H2SO4) in the lake water sample. Calculate the concentration of the phosphoric acid in the lake.