* A 50 gram sample of an unknown metal warms from 18 to 58 after absorbing 800 joules of energy. what is the specific heat of the metal?
*copper has a specific heat of 0.387 j/g degree celsius. what is the mass of a piece of copper that undergoes a
21.0 C temperature change when it absorbs 721 J of energy?
*How many joules of energy must be absorbed to raise the temperature of 21 grams of water from 25 C TO 30 C
Well, well, well, let's dive into these questions like a clown into a ball pit!
For the first one, we need to find the specific heat of the metal. We have a 50-gram sample that warms from 18 to 58 degrees Celsius after absorbing 800 joules of energy. So, the formula we can use is:
q = mcΔT
Where q represents the energy absorbed, m is the mass, c is the specific heat, and ΔT is the change in temperature. Rearranging the formula, we get:
c = q / (m * ΔT)
Plugging in the values, we have:
c = 800 J / (50 g * (58 - 18) °C)
Now, let's calculate it and see what we get.
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For the second question, we're dealing with copper and need to find the mass of the piece that undergoes a 21.0 °C temperature change when it absorbs 721 joules of energy. The formula for finding the mass with specific heat is:
m = q / (c * ΔT)
Plug in the given values, and you'll get your answer.
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Now, onto the third question! We want to know how many joules of energy must be absorbed to raise the temperature of 21 grams of water from 25 °C to 30 °C. The formula is the same as the one we used in the first question:
q = mcΔT
Just plug in the known values, and the answer shall be revealed.
Remember, it's important to make sure all units are consistent throughout the calculations. And if you're ever feeling down, just remember that even equations need a little laughter in their lives! Hope this helps!
To find the specific heat of the metal, we can use the formula:
q = mcΔT
where:
q = energy absorbed (800 J in this case)
m = mass of the metal (50 g)
c = specific heat of the metal (unknown)
ΔT = change in temperature (58°C - 18°C = 40°C)
Plugging in the values, we can rearrange the formula to solve for c:
800 J = (50 g) * c * 40°C
Dividing both sides by (50 g * 40°C) gives:
c = 800 J / (50 g * 40°C)
c ≈ 0.40 J/g°C
Therefore, the specific heat of the metal is approximately 0.40 J/g°C.
To find the mass of the copper, we can rearrange the formula:
q = mcΔT
where:
q = energy absorbed (721 J in this case)
m = mass of the copper (unknown)
c = specific heat of copper (0.387 J/g°C)
ΔT = change in temperature (21.0°C)
Plugging in the values, we can solve for m:
721 J = m * (0.387 J/g°C) * 21.0°C
Dividing both sides by (0.387 J/g°C * 21.0°C) gives:
m = 721 J / (0.387 J/g°C * 21.0°C)
m ≈ 86.44 g
Therefore, the mass of the copper is approximately 86.44 grams.
To find the energy required to raise the temperature of water, we can use the formula:
q = mcΔT
where:
q = energy required (unknown)
m = mass of water (21 g)
c = specific heat of water (4.18 J/g°C)
ΔT = change in temperature (30°C - 25°C = 5°C)
Plugging in the values, we can solve for q:
q = (21 g) * (4.18 J/g°C) * 5°C
q ≈ 439.95 J
Therefore, approximately 439.95 joules of energy must be absorbed to raise the temperature of 21 grams of water from 25°C to 30°C.
To solve the first question, we can use the equation q = mcΔT, where q is the heat absorbed, m is the mass, c is the specific heat, and ΔT is the change in temperature.
In this case, we are given the following information:
- Mass of the unknown metal (m) = 50 grams
- Change in temperature (ΔT) = 58°C - 18°C = 40°C
- Heat absorbed (q) = 800 joules
Plugging these values into the equation, we get:
800 = (50 grams) * c * 40°C
To solve for the specific heat of the metal (c), divide both sides of the equation by (50 grams * 40°C):
c = 800 joules / (50 grams * 40°C)
Simplifying, c = 0.4 joules/gram°C.
Therefore, the specific heat of the metal is 0.4 joules/gram°C.
For the second question, we can use the same formula, q = mcΔT, and rearrange it to solve for mass (m).
Given:
- Specific heat of copper (c) = 0.387 j/g°C
- Change in temperature (ΔT) = 21°C
- Heat absorbed (q) = 721 joules
Plugging in these values, we have:
721 = (m grams) * 0.387 j/g°C * 21°C
To solve for the mass of the copper (m), divide both sides of the equation by (0.387 j/g°C * 21°C):
m = 721 joules / (0.387 j/g°C * 21°C)
Simplifying, m = 92.9 grams.
Therefore, the mass of the piece of copper is 92.9 grams.
Lastly, for the third question, we can again use the formula q = mcΔT.
Given:
- Mass of water (m) = 21 grams
- Change in temperature (ΔT) = 30°C - 25°C = 5°C
- Specific heat of water (c) = 1 calorie/gram°C or 4.18 joules/gram°C (approximately)
Plugging in these values, we can choose the specific heat value as per the units used:
If using calories:
q = (21 grams) * 1 calorie/gram°C * 5°C = 105 calories
If using joules:
q = (21 grams) * 4.18 joules/gram°C * 5°C = 439.53 joules (approximately)
Therefore, the number of joules of energy required to raise the temperature of 21 grams of water from 25°C to 30°C is approximately 439.53 joules.
800J = mass x specific heat x (Tfinal-Tinitial). Substitute and solve for sp.h.
721 = mass Cu x sp.h. Cu x delta T.
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)