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WGU D425 Introduction to Chemistry -PA and
OA EXAM LATEST TESTBANK 2025 UPDATE
WITH COMPLETE QUESTIONS AND
CORRECTLY WELL DEFINED
ANSWERS 100%GUARANTEED PASS!!!
\\\ WGU D425 Introduction to Chemistry -PA
and
what mass of hydrogen peroxide must decompose to produce 48.64g of
water?
2H2O2-> O2+ 2H2O
Given 48.64g H2O
Find g H2O2 -ANSWER-g H2O -> mol H2O -> mol H2O2 -> g H2O2
1. molar mass of H2O 2. mol: mol #. molar mass of H2O2
48.6g H2O (1 mol H2O/18.02g H2O) (2mol H2O2/2mol H2O) (34.02g H2O2/
1mol H2O2)=
48.64x1x2x34.03/18.02x2x1= 91.83g H2O2
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How many molecules of carbon dioxide are required to react with 174g of
carbon monoxide?
2Co+ O2 -> 2CO2
1. g CO -> 2. mol CO2 -> molecules CO2
1. molar mass of CO 2. mol:mol 3. Avogadro's number -ANSWER-174g CO
(1mol CO/28.01g CO) (2 mol CO2/ 2mol CO) (6.022x 10^23 molecules /1 mol
CO2)=
3.74x10^24 molecules CO2
which would be investigated in reaction stoichiometry -ANSWER-the mass
of potassium required to produce an unknown mass of potassium chloride
given the balance equation, how many moles of water H2O are produced by
the complete reaction of 4.0 moles C2H6?
2CH6+ 7O2-> 6H2O+ 4CO2 -ANSWER-
given the balanced equation how many grams of water (H2O=18.015g/mol)
are produced by the complete reaction of 5.22 moles O2
2C2H6+ 7O2-> 6H2O + 4CO2 -ANSWER-
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given the balanced equation how many grams of hydrogen gas
(H2= 2.016 g/mol) are produced by the complete reaction of 489.2 g of
hydrochloric acid (HCL= 36.458 g/mol)
2Na (s) + 2HCl (aq) -> 2NaCl (aq) + H2 (g) -ANSWER-
given the balanced equation how many moles of hydrogen gas (H2) are
produced by the complete reaction of 2.11 x 10^22 atoms of Na
2Na (s) + 2HCl (aq) -> 2NaCl (aq) + H2 (g) -ANSWER-
what happens to a reaction when a limiting reactant in a chemical reaction is
completely used up -ANSWER-the reaction stops
how many moles of potassium chloride are required to yield 250g of oxygen
in the reaction
2KClO3 -> 2KCl+ 3O2 -ANSWER-5.2 mol convert
250.0 grams to moles:
moles=mass/ molar mass, moles = 250.0/32= 7.81 mol
molar ratio btwn KClO3 and O2 is 2:3 the 2=x moles
of KClO3 the 3 = 7.81 mol of O2
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15.62=3x 15.62/3= x cross multiplying to get 5.21 moles =# of
moles of KClO3 req.
if 14.67g of C2H6 is allowed to react with 39.51g of O2 as shown what would
be the limiting reactant molar mass (g/mole)
C2H6= 30.08, O2= 31.998, H2O= 18.015, CO2= 44.08
2C2H6 + 7O2 -> 6H2O + 4CO2 -ANSWER-O2. in order to consume all the
C2H6 we would need 54.62g of O2, we only have 39.51g
what is the maximum amount of product that can be made in a chemical
reaction -ANSWER-theoretical yield is calculated by assuming that all the
limited reagent is converted to product
when 10g of copper and 10g of iodine are mixed, 5g of Cul are made. What is
the percent yield of Cul? the theoretical yield is 15g
2Cu+ I2 -> 2Cul -ANSWER-33% percent yield= actual yield/ theoretical
yield x 100. If 5g are produced, then the percent yield is (5g/ 15g) x 100=
33%
WGU D425 Introduction to Chemistry -PA and
OA EXAM LATEST TESTBANK 2025 UPDATE
WITH COMPLETE QUESTIONS AND
CORRECTLY WELL DEFINED
ANSWERS 100%GUARANTEED PASS!!!
\\\ WGU D425 Introduction to Chemistry -PA
and
what mass of hydrogen peroxide must decompose to produce 48.64g of
water?
2H2O2-> O2+ 2H2O
Given 48.64g H2O
Find g H2O2 -ANSWER-g H2O -> mol H2O -> mol H2O2 -> g H2O2
1. molar mass of H2O 2. mol: mol #. molar mass of H2O2
48.6g H2O (1 mol H2O/18.02g H2O) (2mol H2O2/2mol H2O) (34.02g H2O2/
1mol H2O2)=
48.64x1x2x34.03/18.02x2x1= 91.83g H2O2
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How many molecules of carbon dioxide are required to react with 174g of
carbon monoxide?
2Co+ O2 -> 2CO2
1. g CO -> 2. mol CO2 -> molecules CO2
1. molar mass of CO 2. mol:mol 3. Avogadro's number -ANSWER-174g CO
(1mol CO/28.01g CO) (2 mol CO2/ 2mol CO) (6.022x 10^23 molecules /1 mol
CO2)=
3.74x10^24 molecules CO2
which would be investigated in reaction stoichiometry -ANSWER-the mass
of potassium required to produce an unknown mass of potassium chloride
given the balance equation, how many moles of water H2O are produced by
the complete reaction of 4.0 moles C2H6?
2CH6+ 7O2-> 6H2O+ 4CO2 -ANSWER-
given the balanced equation how many grams of water (H2O=18.015g/mol)
are produced by the complete reaction of 5.22 moles O2
2C2H6+ 7O2-> 6H2O + 4CO2 -ANSWER-
,3|Page
given the balanced equation how many grams of hydrogen gas
(H2= 2.016 g/mol) are produced by the complete reaction of 489.2 g of
hydrochloric acid (HCL= 36.458 g/mol)
2Na (s) + 2HCl (aq) -> 2NaCl (aq) + H2 (g) -ANSWER-
given the balanced equation how many moles of hydrogen gas (H2) are
produced by the complete reaction of 2.11 x 10^22 atoms of Na
2Na (s) + 2HCl (aq) -> 2NaCl (aq) + H2 (g) -ANSWER-
what happens to a reaction when a limiting reactant in a chemical reaction is
completely used up -ANSWER-the reaction stops
how many moles of potassium chloride are required to yield 250g of oxygen
in the reaction
2KClO3 -> 2KCl+ 3O2 -ANSWER-5.2 mol convert
250.0 grams to moles:
moles=mass/ molar mass, moles = 250.0/32= 7.81 mol
molar ratio btwn KClO3 and O2 is 2:3 the 2=x moles
of KClO3 the 3 = 7.81 mol of O2
, 4|Page
15.62=3x 15.62/3= x cross multiplying to get 5.21 moles =# of
moles of KClO3 req.
if 14.67g of C2H6 is allowed to react with 39.51g of O2 as shown what would
be the limiting reactant molar mass (g/mole)
C2H6= 30.08, O2= 31.998, H2O= 18.015, CO2= 44.08
2C2H6 + 7O2 -> 6H2O + 4CO2 -ANSWER-O2. in order to consume all the
C2H6 we would need 54.62g of O2, we only have 39.51g
what is the maximum amount of product that can be made in a chemical
reaction -ANSWER-theoretical yield is calculated by assuming that all the
limited reagent is converted to product
when 10g of copper and 10g of iodine are mixed, 5g of Cul are made. What is
the percent yield of Cul? the theoretical yield is 15g
2Cu+ I2 -> 2Cul -ANSWER-33% percent yield= actual yield/ theoretical
yield x 100. If 5g are produced, then the percent yield is (5g/ 15g) x 100=
33%
