Calculating and explaining energy change Flashcards
What is the unit of measurement for energy?
The joule, J.
How much energy does it take to heat up 1g of water by 1^oC?
4.2 joules of energy.
How many joules is 1 calorie?
4.2 joules.
What is information about the energy provided by food products given in?
Kilocalories (kcal).
What is a chemical change always accompanied by?
An energy change.
What can calorimetry be used to measure?
The relative amounts of energy produced by food or fuels.
What method is used to measure the temperature change that takes place when a fuel burns?
- Place 100g of water in a calorimeter.
- Measure the temperature of the water.
- Find the mass in grams of the fuel to be burned.
- Burn the fuel under the water in the calorimeter for a few minutes.
- Record the new temperature of the water.
- Calculate the temperature change.
- Weigh the fuel.
- Calculate how much fuel has been used.
- Calculate the energy released.
What formula can be used to calculate the energy released by a fuel?
Q = mcΔT where: Q is the energy released in J m is the mass of water being heated, c is 4.2 ΔT is the temperature change.
What happens in a chemical reaction?
New substances are produced.
What must happen for new substances to be produced in a chemical reaction?
The bonds in the reactants must be broken and new bonds are made to form the products.
What does breaking a chemical bond require?
Lots of energy.
What happens once a new chemical bond has been formed?
Energy is given out.
When is a reaction exothermic?
The energy released from forming new bonds is greater than the energy needed to break existing bonds. Energy is transferred to the surroundings.
When is a reaction endothermic?
The energy needed to break existing bonds is greater than the energy released from forming new bonds. Energy is absorbed from the surroundings.
How can the amount of energy produced in a chemical reaction in solution be measured?
By mixing the reactants in an insulated container so that the temperature change is measured before heat is lost to the surroundings.