A 5.00g sample of octane is burned in a bomb calorimeter containing 200g of water. How much energy, in cal, is released if the water temperature increases 6.00C
q = mass H2O x specific heat H2O x delta T.
q = 200g x 1 cal/g x 6.00 = ?
To calculate the amount of energy released, we need to use the equation:
q = m * c * ΔT
Where:
q = energy released (in calories)
m = mass of the water (in grams)
c = specific heat capacity of water (in cal/g°C)
ΔT = change in temperature (in °C)
Given:
Mass of water (m) = 200 g
Change in temperature (ΔT) = 6.00 °C
First, we need to determine the specific heat capacity of water (c). The specific heat capacity of water is approximately 1.00 cal/g°C.
Substituting the values into the equation, we get:
q = 200 g * 1.00 cal/g°C * 6.00 °C
q = 1200 cal
Therefore, when 5.00g of octane is burned in a bomb calorimeter containing 200g of water, the energy released is 1200 calories.
To calculate the energy released in this calorimetry experiment, you need to use the formula:
q = m × c × ΔT
where:
- q is the amount of energy released (in calories)
- m is the mass of the substance (in grams) being heated or cooled (in this case, the water)
- c is the specific heat capacity of the substance (in this case, water)
- ΔT is the change in temperature (in this case, the increase of 6.00°C)
First, let's calculate the heat capacity of the water in the bomb calorimeter using the formula:
C = m × c
where:
- C is the heat capacity of the water
- m is the mass of the water (given as 200g)
- c is the specific heat capacity of water (specific for water = 1 cal/g°C)
C = 200g × 1 cal/g°C
C = 200 cal/°C
Now, we can calculate the amount of energy released using the formula:
q = C × ΔT
q = 200 cal/°C × 6.00°C
q = 1200 cal
Therefore, the energy released in this calorimetry experiment is 1200 calories.