H2O (l) requires the largest amount of energy to raise the temperature of 25.0g H2O of the substance from 15.0 *C to 37.0 *C. Calculate the energy.
Hg (l) has the largest temperature change when 550 g of the substance absorbs 10.7kJ of energy. Calculate the temperature change.
please explain! thank you!
Sure, let's calculate the energy required to raise the temperature of H2O (l) from 15.0°C to 37.0°C.
To do this, we will use the specific heat capacity (c) of water, which is approximately 4.18 J/g°C.
First, we need to find the temperature difference (ΔT) by subtracting the starting temperature from the final temperature:
ΔT = 37.0°C - 15.0°C = 22.0°C
Now, we can calculate the energy using the formula:
Energy = mass (m) × specific heat capacity (c) × temperature change (ΔT).
Plugging in the given values:
Energy = 25.0 g × 4.18 J/g°C × 22.0°C
Calculating this:
Energy = 250 × 4.18 × 22 = 23,210 J
So, it would require approximately 23,210 J of energy to raise the temperature of 25.0 g of H2O (l) from 15.0°C to 37.0°C.
Now let's calculate the temperature change for Hg (l) when 550 g of the substance absorbs 10.7 kJ of energy.
First, we need to convert the energy from kJ to J:
10.7 kJ = 10,700 J
Next, we can use the formula:
Energy = mass (m) × specific heat capacity (c) × temperature change (ΔT).
Since the specific heat capacity of mercury (Hg) is not provided, we can assume it is constant and look it up. The specific heat capacity of mercury is approximately 0.14 J/g°C.
Now, rearranging the formula to solve for temperature change (ΔT):
ΔT = Energy / (mass × specific heat capacity)
Plugging in the given values:
ΔT = 10,700 J / (550 g × 0.14 J/g°C)
Calculating this:
ΔT ≈ 10,700 J / 77 J/°C ≈ 139°C
Therefore, the temperature change for 550 g of Hg (l) when it absorbs 10.7 kJ of energy is approximately 139°C.
To calculate the energy required to raise the temperature of H2O (l) from 15.0 *C to 37.0 *C, we can use the specific heat capacity formula:
q = mcΔT
Where:
q = energy in Joules
m = mass of the substance in grams
c = specific heat capacity of the substance
ΔT = change in temperature (final temperature - initial temperature)
For H2O (l), the specific heat capacity is approximately 4.18 J/g * *C.
Given:
m = 25.0 g
ΔT = 37.0 *C - 15.0 *C = 22.0 *C
c = 4.18 J/g * *C
Substituting the values in the formula:
q = (25.0 g)(4.18 J/g * *C)(22.0 *C)
q = 2,295 J
Therefore, the energy required to raise the temperature of 25.0 g H2O from 15.0 *C to 37.0 *C is 2,295 Joules.
To calculate the temperature change for Hg (l) when 550 g of the substance absorbs 10.7 kJ of energy, we can rearrange the specific heat capacity formula:
q = mcΔT
To solve for ΔT:
ΔT = q / (mc)
Given:
q = 10.7 kJ = 10,700 J
m = 550 g
c = specific heat capacity of Hg (l)
Since the specific heat capacity of Hg (l) was not provided, we can assume it is constant and equal to 0.14 J/g * *C.
Substituting the values in the formula:
ΔT = (10,700 J) / (550 g * 0.14 J/g * *C)
ΔT ≈ 1.32 *C
Therefore, the temperature change for Hg (l) when 550 g of the substance absorbs 10.7 kJ of energy is approximately 1.32 *C.
To calculate the energy required to raise the temperature of a substance, we can use the formula:
q = m * c * ΔT
Where:
q = energy (in joules)
m = mass of the substance (in grams)
c = specific heat capacity of the substance
ΔT = change in temperature (in degrees Celsius)
For the first question:
Given:
m = 25.0 g
ΔT = (37.0 - 15.0) *C = 22.0 *C
To find the specific heat capacity (c) for water, we can use the known value of 4.18 J/(g*C).
Putting the values into the formula:
q = 25.0 g * 4.18 J/(g*C) * 22.0 *C
Calculating:
q = 25.0 g * 4.18 J/(g*C) * 22.0 *C
q = 2299 J
Therefore, the energy required to raise the temperature of 25.0 g of water from 15.0 *C to 37.0 *C is 2299 J.
For the second question:
Given:
m = 550 g
q = 10.7 kJ = 10.7 * 10^3 J
We need to calculate the change in temperature (ΔT). Rearranging the formula above, we have:
ΔT = q / (m * c)
The specific heat capacity of mercury (Hg) is 0.14 J/(g*C).
Plugging the values into the formula:
ΔT = 10.7 * 10^3 J / (550 g * 0.14 J/(g*C))
Calculating:
ΔT = 10,700 J / (77 J/(g*C))
ΔT = 139.0 *C
Therefore, the temperature change of 550 g of mercury when it absorbs 10.7 kJ of energy is 139.0 *C.
H2O.
q = mass x specific heat x (Tfinal-Tinitial)
Solve for q.
Hg.
q = mass x specific heat x delta T.
Solve for delta T.