H2(g) + Reactants O2(g) → yield H₂O(1) unbalanced Products This means one mole of H 2 and one mole of O 2 react to form one mole of H 2 O. We have two moles of hydrogen on the left and two moles of hydrogen on the right. The hydrogen is balanced. BUT take a look at oxygen. We have two moles of oxygen on the left but only one mole of oxygen on the right. Chemical equations must be balanced.

H2(g) + Reactants O2(g) → yield H₂O(1) unbalanced Products This means one mole of H 2 and one mole of O 2 react to form one mole of H 2 O. We have two moles of hydrogen on the left and two moles of hydrogen on the right. The hydrogen is balanced. BUT take a look at oxygen. We have two moles of oxygen on the left but only one mole of oxygen on the right. Chemical equations must be balanced.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In a reaction, 1 mole of silver nitrate combines with 1 mole of sodium chloride. AgNO3 + NaCl Which statement about the product is justified by the law of conservation of mass? There will be five atoms in the product. There will be two molecules in the product. There will be 1 mole of silver (Ag) in the product. There will be 2 moles of sodium (Na) in the product.
Potassium chlorate decomposes to potassium chloride and oxygen, as shown in the equation below. 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g) Which of the following sentences is a correct expression for a relationship between substances in this reaction? a. One mole of potassium chlorate decomposes into one mole of potassium chloride and one mole of oxygen. b. Two moles of potassium chlorate decompose into two moles of potassium chloride and three moles of oxygen. c. Two liters of potassium chlorate decompose into two liters of potassium chloride and three liters of oxygen. d. Two grams of potassium chlorate decompose into two grams of potassium chloride and three grams of oxygen.
Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced and contains state symbols after every reactant and product. HBr (aq) + H2O(l) → ローロ х G
Consider the following balanced chemical equation: 2 Na(s) + Cl2 (3) →2 NaCl(s) If 4 moles of sodium chloride are produced, how many moles of chlorine gas are used up? 2.0 mol O 1.0 mol 0.5 mol more information is needed
The reaction of carbon dioxide to form carbon monoxide and oxygen is what type of reaction? 2CO2(g) → 2CO(g) + O2(g) decomposition combustion oxidation combination single replacement
The "barking dog" reaction is an exciting combustion reaction that generates a bright blue flame because sulfur is produced during the reaction (sulfur burns blue!). At the end of the reaction, a "woosh" sound is made which sounds like a dogs bark (hence the name of the reaction). Assume the reaction is carried out in a closed container. CS₂2 +4N₂O CO₂ + SO₂ + S + 4N₂ Note: the equation is balanced How many moles of CO₂ can you generate if you were to carry out the reaction with 8.28 g CS₂?
the balance chemical equation is P4(s) + 6Cl2(g) -> 4PCl3(g). what is the mass in grams of phosphorus trichloride that can be formed from 150.1 grams of P4 based on the balanced chemical equation?
Write a balanced chemical equation based on the following description: solid sodium reacts with chlorine gas to produce solid sodium chloride. Na(s)+Cl2(g)_
If you wanted to produce 4 moles of SO3 gas, how many moles of SO2 would you need to react? (Assume an unlimited supply of O2 gas.) 2 SO₂ (g) + O₂(g) →2 SO, (g)
Using the balanced chemical equation below, calculate the moles of carbon dioxide, CO2, produced by the complete decomposition of 1.75 moles of calcium carbonate, CaCO3. CaCO3(s) → CaO(s) + CO2(g)
Oxygen is a product of the decomposition of mercury(II) oxide as shown below. 2 HgO(s) → 2 Hg(ℓ) + O₂(g) In the last question, you determined that you started with 0.0152 moles of HgO. How many moles of O₂ gas will be formed in this reaction?
Use the chemical equation below to determine how many moles of ammonia will be produced from 4 moles of nitrogen gas. Assume that there is enough H2 for all of the N2 to be converted to NH3. N2 + 3H2 ---> 2NH3