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# 1.29 Calculating masses

Chemical equations are a useful shorthand way of describing the changes that take place when a chemical reaction happens.  Word equations can be helpful for example :

It is often more helpful to use the chemical formulae of the reactants since the formulae show the actual elements involved:

For example if you were predicting a word equation for when methane burns in oxygen you might suggest:

what's wrong with this?

This is wrong of course because methane is not a single element, it is a compound of carbon and hydrogen (CH4). When it burns in a plentiful supply of oxygen (O2) the carbon in methane becomes carbon dioxide (CO2) and the hydrogen becomes water (H2O). This is more easily shown as a symbol equation:

#### Students should:

1.29 calculate reacting masses using experimental data and chemical equations

Use the animation to see how to balance the equation for the combustion of methane.

Notice that when it is balanced, the equation shows that the total mass of the reactants is equal to the total mass of the products.

The law of conservation of mass states that the mass of the products in a chemical reaction must equal the mass of the reactants

We use this idea throughout the course.

#### 1.29 Activity 1. Masses reacting

​The video here shows a classic reaction where hydrogen gas (H2) is used to remove oxygen from copper (II) oxide (CuO). The reactants are therefore hydrogen and copper oxide.  The products are water and copper.

Study the  video closely. You will see that the black copper oxide slowly becomes copper coloured as the oxygen is removed from it. The water produced in this reaction leaves the tube as vapour and so the mass of the tube decreases as the reaction continues:

balanced equations and relative masses allow us to predict mass changes

#### 1.29 Keep it in proportion

The combustion of methane in oxygen produces carbon dioxide gas as well as water vapour. This exercise allows us to calculate the "carbon footprint" produced by the burning of this fossil fuel.

Use the equation and the relative mass data in the video to calculate the following:

the mass of:

1. carbon dioxide produced when 32g methane is burnt in excess oxygen?
2. water produced when 1.6 g methane is burnt in excess oxygen?
3. oxygen required for the complete combustion of 640g methane?
4. carbon dioxide produced by the complete combustion of 1g of methane
5. carbon dioxide produced by the complete combustion of 1 tonne of methane?
The method shown here uses the ideas of proportionality to calculate the various quantities involved:
1. 88g of carbon dioxid
2. 3.6g water
3. 2560g oxygen
4. 2.75g carbon dioxide
5. 2.75 tonnes carbon dioxide

Other methods use the idea of moles to perform the calculations .

using proportionality

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