(a)
Interpretation:
The correct element and/or compound symbols, formulas, and coefficients needed to produce complete, balanced equation has to be given.
(a)
Answer to Problem 2.35QP
Explanation of Solution
The product in the given chemical equation is Lithium chloride. Hence, the starting material has to be Lithium and Chlorine.
To balance the chemical equation, coefficient 2 has to be added before
(b)
Interpretation:
The correct element and/or compound symbols, formulas, and coefficients needed to produce complete, balanced equation has to be given.
(b)
Answer to Problem 2.35QP
Explanation of Solution
The product in the given chemical equation is sodium sulfide. Hence, the starting material has to be Sodium and Sulfur.
To balance the chemical equation, coefficient 16 before sodium, and coefficient 8 has to be added before
(c)
Interpretation:
The correct element and/or compound symbols, formulas, and coefficients needed to produce complete, balanced equation has to be given.
(c)
Answer to Problem 2.35QP
Explanation of Solution
The product in the given chemical equation is aluminium iodide. Hence, the starting material has to be Aluminium and Iodine.
To balance the chemical equation, coefficient 3 before aluminium and iodine. Coefficient 2 has to be added before
(d)
Interpretation:
The correct element and/or compound symbols, formulas, and coefficients needed to produce complete, balanced equation has to be given.
(d)
Answer to Problem 2.35QP
Explanation of Solution
The product in the given chemical equation is Barium nitride. Hence, the starting material has to be Barium and Nitrogen.
To balance the chemical equation, coefficient 3 has to be added before barium. Hence, the equation can be written as,
(e)
Interpretation:
The correct element and/or compound symbols, formulas, and coefficients needed to produce complete, balanced equation has to be given.
(e)
Answer to Problem 2.35QP
Explanation of Solution
The product in the given chemical equation is
To balance the chemical equation, start balancing phosphorous first. In the product side coefficient 4 has to be added and in the reactant side, coefficient 5 has to be added before phosphorous. Hence, the equation can be written as,
Now start to balance vanadium. This is done by adding coefficient 12 before vanadium in the reactant side. The balanced equation can be written as,
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Chapter 2 Solutions
General Chemistry - Standalone book (MindTap Course List)
- Assign each of the following molecular descriptions for a pure substance to the categories (1) must be an element, (2) must be a compound, or (3) could be an element or a compound. a. Molecules are triatomic. b. Molecules contain only one kind of atom. c. Molecules are heteroatomic. d. Molecules are both homoatomic and diatomic.arrow_forwardIndicate whether each of the following statements is true or false. a. Compounds can be separated into their constituent elements by chemical means. b. Elements can be separated into their constituent compounds by physical means. c. A compound must contain at least two elements. d. A compound is a physical mixture of different elements.arrow_forwardWater and sodium chloride are both considered substances as well as compounds, but water exists as molecules while sodium chloride does not. (i) Explain this difference in the behavior of water and sodium chloride. As part of your explanation, (ii) define the terms substance, molecule, and compound.arrow_forward
- Matter is neither created nor destroyed in a chemical reaction. Thus, the mass of the products of a chemical reaction must be equal to the mass of the starting materials. Formally, this concept is called the law of conservation of mass. A sample of sodium reacts completely with 0.426 kg k g of chlorine, forming 702 g g of sodium chloride. What mass of sodium reacted?arrow_forwardClassify the statements pertaining to elements and compounds as either true or false. True False Compounds must contain at least [wo elements. Compounds are pure substances whereas elements are mixtures Compounds cannot be broken down further by processes such as filtration. Compounds may be broken down into simpfer substances through: chemical processes. A compound is a physical mixture of simpler substances.arrow_forwardA large number of atoms of the same kind is called an element a compound a mixture Depends on the number of atoms None of thesearrow_forward
- Which of the following statements about compounds and molecules are true? not all compounds are molecules all molecules are compounds not all molecules are compounds all compounds are moleculesarrow_forwardPresent 5 chemical reactions involved in biological and industrial processes affecting life and the environment. Give the reactants and products from the chemical reactions. Write the chemical formula of each of the reactants and products.arrow_forwardCounting Atoms The formula for a compound indicates the elements that make up the compound and the number of atoms of each element present in the compound. These numbers of atoms are indicated by the use of small numbers called subscripts. Sometimes groups of atoms act as a single atom. When a subscript appears outside the parentheses, it indicates that all the elements inside the parentheses should be multiplied by that subscript. For example, the formula Fe(OH)3 indicates the combination of 1 atom of iron, Fe, 3 atoms of oxygen, O, and 3 atoms of hydrogen, H. In the following examples, list each element in the compound and the number of atoms of each element present. The first example has been done for you. You may already be familiar with some of the compounds. FIX ANY WRONG PROBLEMS! **Use the periodic table link to help you identify the elements used NAME USE FORMULA ATOMS IN FORMULA Calcium Carbonate Limestone CaCO3 Ca=1 calcium C = 1…arrow_forward
- Classify substance as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous. CARBON MONOXIDEarrow_forwardMatter is neither created nor destroyed in a chemical reaction. Thus, the mass of the products of a chemical reaction must be equal to the mass of the starting materials. Formally, this concept is called the law of conservation of mass. When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 16.8 g g of carbon were burned in the presence of 59.1 g of oxygen, 14.3 g of oxygen remained unreacted. What mass of carbon dioxide was produced?arrow_forwardThe Law of Conservation of Mass states that matter is not gained or lost in a chemical reaction. Which of the following correctly restates this law? In a chemical reaction Matter is gained and lost but energy is conserved. The amount of mass is equal to the sum of the reactants and products. Matter is gained and lost in depending on how much energy is added. The amount of mass of the reactants will equal the mass of the productsarrow_forward
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