How many joules are needed to hear 125.0g of ive at -35.0C to steam at 130.0 C?
heat= heat to warm ice to OC+heat to melt ice at 0C+heat to warm water from 0 to 100C + heat to vaporize water at 100C + heat to heat steam from 100 to 130C
add all of those, show your work, and I will gladly check.
To calculate the amount of energy required to heat a substance, you can use the formula:
q = m * C * ΔT
where:
q is the heat energy (in joules)
m is the mass of the substance (in grams)
C is the specific heat capacity of the substance
ΔT is the change in temperature (in degrees Celsius)
Given:
m = 125.0g (mass of ice)
ΔT = 130.0°C - (-35.0°C) = 165.0°C (change in temperature)
First, we need to calculate the heat energy required to heat the ice from -35.0°C to 0°C (melting point of ice).
q1 = m * Cice * ΔT1
We can use the specific heat capacity of ice (Cice) which is 2.09 J/g°C.
ΔT1 = 0°C - (-35.0°C) = 35.0°C
q1 = 125.0g * 2.09 J/g°C * 35.0°C
q1 = 9178.75 J
Next, we need to calculate the heat energy required to melt the ice.
q2 = m * ΔHfusion
The latent heat of fusion for water (ΔHfusion) is 334 J/g.
q2 = 125.0g * 334 J/g
q2 = 41750 J
Now, we need to calculate the heat energy required to heat the water from 0°C to 100°C.
q3 = m * Cwater * ΔT2
We can use the specific heat capacity of water (Cwater), which is 4.18 J/g°C.
ΔT2 = 100°C - 0°C = 100°C
q3 = 125.0g * 4.18 J/g°C * 100.0°C
q3 = 52250 J
Finally, we need to calculate the heat energy required to vaporize the water.
q4 = m * ΔHvaporization
The latent heat of vaporization for water (ΔHvaporization) is 2260 J/g.
q4 = 125.0g * 2260 J/g
q4 = 282500 J
To find the total heat energy required, we add up all the calculated values:
Total heat energy = q1 + q2 + q3 + q4 =
9178.75 J + 41750 J + 52250 J + 282500 J =
388678.75 J
Therefore, approximately 388678.75 joules are needed to heat 125.0 grams of ice at -35.0°C to steam at 130.0°C.
To calculate the amount of energy (in joules) required to heat a substance, we can use the formula:
q = m * c * ΔT
where:
- q represents the amount of energy
- m represents the mass of the substance
- c represents the specific heat capacity of the substance
- ΔT represents the change in temperature
First, we need to calculate the energy required to heat the ice from -35.0°C to 0°C. Since ice has a specific heat capacity of 2.09 J/g°C, we can use the formula:
q_ice = m_ice * c_ice * ΔT_ice
where:
- q_ice represents the energy required to heat the ice
- m_ice is the mass of the ice
- c_ice is the specific heat capacity of ice (2.09 J/g°C)
- ΔT_ice is the change in temperature (0 - (-35.0) = 35.0°C)
Let's substitute the values we have:
q_ice = 125.0g * 2.09 J/g°C * (0 - (-35.0)°C)
= 125.0g * 2.09 J/g°C * 35.0°C
Next, we need to calculate the energy required to convert the ice at 0°C to water at 0°C. This is known as the heat of fusion, and for water, it is 334 J/g. The formula is similar:
q_fusion = m_ice * ΔH_fusion
where:
- q_fusion represents the energy required to convert ice to water
- m_ice is the mass of the ice
- ΔH_fusion is the heat of fusion for water (334 J/g)
Let's substitute the values we have:
q_fusion = 125.0g * 334 J/g
Now, we need to calculate the energy required to heat the water from 0°C to 100°C. The specific heat capacity of water is 4.18 J/g°C. Again, using the formula:
q_water = m_water * c_water * ΔT_water
where:
- q_water represents the energy required to heat water
- m_water is the mass of the water (which is the same as the mass of the ice)
- c_water is the specific heat capacity of water (4.18 J/g°C)
- ΔT_water is the change in temperature (100 - 0 = 100°C)
Let's substitute the values we have:
q_water = 125.0g * 4.18 J/g°C * 100.0°C
Finally, we need to calculate the energy required to convert water at 100°C to steam at 130°C. This is known as the heat of vaporization, and for water, it is 2260 J/g. Using the formula:
q_vaporization = m_water * ΔH_vaporization
where:
- q_vaporization represents the energy required to convert water to steam
- m_water is the mass of the water
- ΔH_vaporization is the heat of vaporization for water (2260 J/g)
Let's substitute the values we have:
q_vaporization = 125.0g * 2260 J/g
Now, we add up all the values to find the total energy required:
Total energy = q_ice + q_fusion + q_water + q_vaporization
If you substitute the values into the formulas and perform the calculations, you will find the answer in joules.