Stoichiometry Practice Problem Michelle Lamary. Question How many grams of water are produced when 5.14 grams of Hydrogen Nitrite is reacted with Barium.

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Presentation transcript:

Stoichiometry Practice Problem Michelle Lamary

Question How many grams of water are produced when 5.14 grams of Hydrogen Nitrite is reacted with Barium Hydroxide?

Write a Complete and Balanced Equation 2H(NO 2 ) + Ba(OH) 2  2H 2 O + Ba(NO 2 ) 2

Draw a Column for Each Chemical 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) 2

Write the Amount Given in the Appropriate Column 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g

Convert the Given Amount Into Moles 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g g g +2(15.999) g g 5.14 g x 1 mole g.109 moles

Find Moles for Each of the Other Chemicals 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g Moles? g g +2(15.999) g g 5.14 g x 1 mole g.109 moles

In Each of the Columns Write the Moles of Given (x) a Fraction 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g.109 moles x ?/? = g g +2(15.999) g g 5.14 g x 1 mole g.109 moles

The Numerator of the Fraction is the Coefficient of the That Column 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g.109 moles x 1/? =.109 moles x 2/? =.109 moles x 1/? = g g +2(15.999) g g 5.14 g x 1 mole g.109 moles

The Denominator of the Fraction is the Coefficient of the Given Column 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g.109 moles x ½ =.109 moles x 2/2 =.109 moles x ½ = g g +2(15.999) g g 5.14 g x 1 mole g.109 moles

Do Math and Label as Moles 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g.109 moles x ½ =.109 moles x 1 =.109 moles x ½ = g g +2(15.999) g g.0545 moles. 109 moles.0545 moles 5.14 g x 1 mole g.109 moles

Convert All Moles Into Grams 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g.109 moles x ½ =.109 moles x 1 =.109 moles x ½ = g g +2(15.999) g g.0545 moles. 109 moles.0545 moles g + 2(15.999) g + 2(1.0079) g g 2(1.0079) g g g g + 2(14.007) g + 4(15.999) g g 5.14 g x 1 mole g.0545 moles x g 1 1 mole.109 moles x g 1 1 mole.0545 moles x g 1 1 mole.109 moles 9.34 g1.96 g12.5 g

Verify the Law of Conservation and Mass 2H(NO 2 )+ Ba(OH) 2  2H 2 O +Ba(NO 2 ) g.109 moles x ½ =.109 moles x 1 =.109 moles x ½ = g g +2(15.999) g g.0545 moles. 109 moles.0545 moles g + 2(15.999) g + 2(1.0079) g g 2(1.0079) g g g g + 2(14.007) g + 4(15.999) g g 5.14 g x 1 mole g.0545 moles x g 1 1 mole.109 moles x g 1 1 mole.0545 moles x g 1 1 mole.109 moles 9.34 g1.96 g12.5 g g14.46 g

Answer 1.96 grams of water (H 2 O) are produced when 5.14 grams of Hydrogen Nitrite [H(NO 2 )] is reacted with Barium Hydroxide [Ba(OH) 2 ].