Chemical Equation Balancer - CuO + H2 = Cu + H2O - ChemicalAid

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Balanced Chemical Equation

CuO + H2 → Cu + H2O Reaction Info Balance Another Equation Thermodynamics Step-by-Step Solution Practice Balancing

Reaction Information

Word Equation

Copper(Ii) Oxide + Dihydrogen = Copper + Water

CuO + H2 = Cu + H2O is a Single Displacement (Substitution) reaction where one mole of Copper(Ii) Oxide [CuO] and one mole of Dihydrogen [H2] react to form one mole of Copper [Cu] and one mole of Water [H2O]

Reaction Type

Single Displacement (Substitution)

• Redox

Redox (Oxidation-Reduction) Reaction

CuO + H2 = Cu + H2O might be a redox reaction.

Reactants

• Copper(Ii) Oxide - CuO

  Cupric Oxide Cuprum Oxydatum Nigrum Cu(Ii) Oxide Copper Oxide Copper Monoxide CuO Molar Mass CuO Bond Polarity CuO Oxidation Number

• Dihydrogen - H2

  Molecular Hydrogen Hydrogen Molecule Hydrogen Hydrogen Gas Molecular Hydrogen Gas H₂ H2 Molar Mass H2 Bond Polarity H2 Oxidation Number

Products

• Copper - Cu

  Cuprum Element 29 Paragard T 380A Tatum-T Cu-7 Cu Molar Mass Cu Oxidation Number

• Water - H2O

  Hydroxic Acid H₂O [Oh2] Aqua Pure Water Hydrogen Oxide Oxidane Dihydrogen Oxide H2O Molar Mass H2O Oxidation Number

Show Chemical Structure Image

Thermodynamics

Thermodynamics of the reaction can be calculated using a lookup table.

Choose Compound States CuO (s)CuO H2 (g)H2 Cu (g)Cu (s)Cu H2O (g)H2O (l)H2O Change States Enthalpy Calculator

Is the Reaction Exothermic or Endothermic?

CuO (s)	1 mol	-157.3184 kJ/mol	157.3184 kJ
H2 (g)	1 mol	0 kJ/mol	-0 kJ
Cu (g)	1 mol	338.31824 kJ/mol	338.31824 kJ
H2O (g)	1 mol	-241.818464 kJ/mol	-241.818464 kJ
ΣΔH°f(reactants)	-157.3184 kJ
ΣΔH°f(products)	96.499776 kJ
ΔH°rxn	253.818176 kJ

ΣΔH°f(products) > ΣΔH°f(reactants), so CuO + H2 = Cu + H2O is endothermic (absorbs heat). Entropy Calculator

Is the Reaction Exoentropic or Endoentropic?

ΔS = Sproducts - Sreactants. If ΔS < 0, it is exoentropic. If ΔS > 0, it is endoentropic.

CuO (s)	1 mol	42.63496 J/(mol K)	-42.63496 J/K
H2 (g)	1 mol	130.586824 J/(mol K)	-130.586824 J/K
Cu (g)	1 mol	166.27216 J/(mol K)	166.27216 J/K
H2O (g)	1 mol	188.715136 J/(mol K)	188.715136 J/K
ΣΔS°(reactants)	173.221784 J/K
ΣΔS°(products)	354.987296 J/K
ΔS°rxn	181.765512 J/K

ΣΔS°(products) > ΣΔS°(reactants), so CuO + H2 = Cu + H2O is endoentropic (increase in entropy). Gibbs Free Energy Calculator

Is the Reaction Exergonic or Endergonic?

ΔG = Gproducts - Greactants. If ΔG < 0, it is exergonic. If ΔG > 0, it is endergonic.

CuO (s)	1 mol	-129.704 kJ/mol	129.704 kJ
H2 (g)	1 mol	0 kJ/mol	-0 kJ
Cu (g)	1 mol	298.61208 kJ/mol	298.61208 kJ
H2O (g)	1 mol	-228.588656 kJ/mol	-228.588656 kJ
ΣΔG°(reactants)	-129.704 kJ
ΣΔG°(products)	70.023424 kJ
ΔG°rxn	199.727424 kJ

ΣΔG°(products) > ΣΔG°(reactants), so CuO + H2 = Cu + H2O is endergonic (absorbs energy).

Reaction Expressions

Equilibrium Constant & Reaction Quotient Kc or Q = ( [Cu] [H2O] ) / ( [CuO] [H2] )(assuming all reactants and products are aqueous. substitutue 1 for any solids/liquids, and Psubstance for gases.) Rate of Reaction rate = -(Δ[CuO] / Δt) = -(Δ[H2] / Δt) = (Δ[Cu] / Δt) = (Δ[H2O] / Δt)(assuming constant volume in a closed system and no accumulation of intermediates or side products) Calculate Reaction Stoichiometry Calculate Limiting Reagent Chemical Equation Balancer 🛠️ Balance Equation ➜

Instructions

To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. The balanced equation will appear above.

• Use uppercase for the first character in the element and lowercase for the second character. Examples: Fe, Au, Co, Br, C, O, N, F.
• Ionic charges are not yet supported and will be ignored.
• Replace immutable groups in compounds to avoid ambiguity. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will.
• Compound states [like (s) (aq) or (g)] are not required.
• You can use parenthesis () or brackets [].

How To Balance Equations

Balance any equation or reaction using this chemical equation balancer! Find out what type of reaction occured.

Read our article on how to balance chemical equations or ask for help in our chat.

Examples

• Copper(Ii) Oxide + Dihydrogen = Copper + Water
• Cu + H2O + CO + O2 = Cu(OH) + CuCO
• Cu + H2O + CO + O2 = Cu(OH) + CuCO3
• Cu + H2O + CO2 + O2 = (CuOH)2CO3
• Cu + H2O + CO2 + O2 = Cu(OH)2 + CuCO
• Cu + H2O + CO2 + O2 = Cu(OH)2 + CuCO2 + H2O + CO2
• Cu + H2O + CO2 + O2 = Cu(OH)2 + CuCO3
• Cu + H2O + CO2 + O2 = Cu(OH)2CuCO3
• Cu + H2O + CO2 + O2 = Cu2(CO3)(OH)2
• O2 + CuO = CuO2
• C2H3O2Cl + NH3 = C2H5NO2 + HCl
• CaO + PbO = Ca + O2Pb
• Fe2O3 + (3C) = (4Fe) + (3CO2)
• Recently Balanced Equations

Balance CuO + H2 = Cu + H2O Using the Algebraic Method

To balance the equation CuO + H2 = Cu + H2O using the algebraic method step-by-step, you must have experience solving systems of linear equations. The most common methods are substitution/elimination and linear algebra, but any similar method will work.

Step 1: Label Each Compound With a Variable

Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients.

a CuO + b H2 = c Cu + d H2O

Step 2: Create a System of Equations

Create an equation for each element (Cu, O, H) where each term represents the number of atoms of the element in each reactant or product.

Cu: 1a + 0b = 1c + 0d O: 1a + 0b = 0c + 1d H: 0a + 2b = 0c + 2d

Step 3: Solve For All Variables

Use substitution, Gaussian elimination, or a calculator to solve for each variable.

Using Substitution or Elimination

• 1a - 1c = 0
• 1a - 1d = 0
• 2b - 2d = 0

Using Linear Systems / Algebra

Use your graphing calculator's rref() function (or an online rref calculator) to convert the following matrix into reduced row-echelon-form:

[ 1 0 -1 0 0] [ 1 0 0 -1 0] [ 0 2 0 -2 0] The resulting matrix can be used to determine the coefficients. In the case of a single solution, the last column of the matrix will contain the coefficients. Convert to RREF and Solve Step-by-Step

Simplify the result to get the lowest, whole integer values.

• a = 1 (CuO)
• b = 1 (H2)
• c = 1 (Cu)
• d = 1 (H2O)

Step 4: Substitute Coefficients and Verify Result

Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.

CuO + H2 = Cu + H2O

Reactants	Products
Cu	1	1	✔️
O	1	1	✔️
H	2	2	✔️

Since there is an equal number of each element in the reactants and products of CuO + H2 = Cu + H2O, the equation is balanced.

Balance CuO + H2 = Cu + H2O Using Inspection

The law of conservation of mass states that matter cannot be created or destroyed, which means there must be the same number atoms at the end of a chemical reaction as at the beginning. To be balanced, every element in CuO + H2 = Cu + H2O must have the same number of atoms on each side of the equation. When using the inspection method (also known as the trial-and-error method), this principle is used to balance one element at a time until both sides are equal and the chemical equation is balanced.

Step 1: Count the number of each element on the left and right hand sides

Reactants (Left Hand Side)			Products (Right Hand Side)
Reactants	Products
CuO	H2	Total	Cu	H2O	Total
Cu	1	1	1	1	✔️
O	1	1	1	1	✔️
H	2	2	2	2	✔️

The number of atoms of each element on both sides of CuO + H2 = Cu + H2O is equal which means that the equation is already balanced and no additional work is needed.

Practice Balancing

CuO - + + H2 - + = Cu - + + H2O - +

Reactants	Products
Cu	1	1	✔️
O	1	1	✔️
H	2	2	✔️

Hint: The sum of the balanced coefficients is 4. See Step-By-Step Solution

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