"Simple Calculation Using Chemical Equations" Chemical Equations PPT Courseware 7

Description

"Simple Calculation Using Chemical Equations" Chemical Equations PPT Courseware 7

Review questions

Take the combustion of magnesium in air as an example to illustrate one of the meanings of the chemical equation.

Mass ratio between reactants and products in magnesium combustion reaction in air

1. Calculate the mass of the product if the mass of the reactants is known.

Example 1: How many grams of oxygen can be obtained by heating and decomposing 6.3 g of potassium permanganate?

Solution: Suppose that 6.3 g of potassium permanganate is decomposed by heating, and the mass of oxygen that can be obtained is x.

2. If the mass of the product is known, find the mass of the reactant.

Example 2: In industry, quicklime (CaO) and carbon dioxide can be produced by calcining limestone (CaCO3) at high temperature. If 5.6 t of calcium oxide is to be produced, how many tons of calcium carbonate are needed?

Class exercises

Hydrogen burns in chlorine to form hydrogen chloride gas. What is the mass of chlorine required to burn 100g of hydrogen? What is the mass of hydrogen chloride gas produced?

1: A certain pure substance X burns completely in air. The chemical equation of the reaction is:

X + 3O2 = 2CO2 + 2H2O, try to deduce the chemical formula of X______.

2. If 2X + 3O2 = 2CO2 + 4H2O, try to deduce the chemical formula of X _______.

3. Heat a mixture containing 3 grams of potassium chlorate and 1 gram of manganese dioxide for a while, then cool it. The mass of the residual solid is weighed as 3.04 grams. According to the law of conservation of mass, how many grams of oxygen is produced? What substances are contained in the solid residue? What is the mass?

Idea: The mass of the solid material is reduced during the reaction. Originally 3 grams + 1 gram = 4 grams. After heating for a while, the remaining solid material is 3.04 grams. Why is the mass of the solid material reduced? How much relief? What substance's mass is being reduced?

4. About the conversion between mass and volume

How many grams of magnesium oxide can be produced when a sufficient amount of magnesium ribbon is fully burned with 11.2 liters of oxygen (density 1.43g/L) under standard conditions?

Note: If the volume is known or the volume needs to be calculated, the density formula must be used to convert it into mass before substituting it.

Medical treatment requires 180 kilograms of oxygen. If it is produced by electrolyzing water, how many kilograms of hydrogen can be obtained at the same time? What volume does this hydrogen occupy under standard conditions? (ρH2=0.09g/L)

Mass of gas = Volume of gas × Density of gas

practise

1. When the following substances of equal mass are completely burned in oxygen, the one that consumes the most oxygen is ( )

A. Hydrogen gas b. Red phosphorus c. Sulfur D. iron

2. Equal masses of iron and zinc react with a sufficient amount of dilute hydrochloric acid respectively. The known chemical equations of the reactions are: Fe+2HCl=FeCl2+H2↑, Zn+2HCl=ZnCl2+H2↑. Then the mass of hydrogen produced is ( )

A. equal b. Iron is greater than zinc C. Iron is smaller than zinc D. Can't compare

3. When 15.8g potassium permanganate is heated and 1.6g oxygen is produced, the composition of the solid residue is ( )

A. K2MnO4 and MnO2 B． KMnO4, K2MnO4 and MnO2

C. KMnO4 and MnO2 D. KMnO4 and K2MnO4

4. Which of the following statements about hydrogen burning in oxygen is correct ( )

A. The reaction of 16g ​​hydrogen and 2g oxygen can produce 18g water

B． The reaction of 9g hydrogen and 9g oxygen can produce 18g water

C. The reaction of 1g hydrogen and 8g oxygen can produce 9g water

D． The reaction of 8g hydrogen and 1g oxygen can produce 9g water

Several methods in chemical reaction calculations

1. Use chemical formulas to calculate

The complete transformation of an element in a substance into another substance

2. Calculate using chemical equations

If the mass of any substance is known, the mass of other substances can be found

3. Calculation using the law of conservation of mass

Only one of all reactants and products is unknown

Keywords: chemical equation teaching courseware, simple calculation teaching courseware using chemical equations, PPT courseware download for the first volume of the ninth grade chemistry of the People's Education Edition, downloading the ninth grade chemistry slide courseware, downloading chemical equation PPT courseware, simple calculation using chemical equation PPT courseware Download, .PPT format;

For more information about the "Chemical Equations Simple Calculations Using Chemical Equations" PPT courseware, please click on the Chemical Equations ppt Simple Calculations Using Chemical Equations ppt tag.

"Simple Calculation Using Chemical Equations" Chemical Equations PPT Courseware 6:

"Simple Calculations Using Chemical Equations" Chemical Equations PPT Courseware 6 Learning Objectives 1. Further understand the meaning of chemical equations, and be able to perform simple calculations based on correctly writing chemical equations. 2. Master the ideas and rules for calculating chemical equations..

"Simple Calculation Using Chemical Equations" Chemical Equations PPT Courseware 5:

"Simple Calculation Using Chemical Equations" Chemical Equations PPT Courseware 5 Learning Objectives 1. On the basis of understanding the meaning of chemical equations, master the calculation of the mass of reactants and products. 2. Master the calculation of chemical equations through relevant chemical equation calculations..

"Simple Calculation Using Chemical Equations" Chemical Equations PPT Courseware 4:

"Simple Calculation Using Chemical Equations" Chemical Equations PPT Courseware 4 Review questions: 1. Do you know the meaning of chemical equations? (1), indicating the reactants, products and reaction conditions. (2), represents the number of particles between each reactant and product..

File Info

Update Time: 2024-10-02

This template belongs to Chemistry courseware People's Education Press Ninth Grade Chemistry Volume 1 industry PPT template

Preview