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Solid iron a specific heat of 0.444 J/g°C. If 75 calories of energy were removed from a piece of iron, and the temperature of the iron went from 21.4°C to -25.2°C, what was the mass of the iron?
When you look at the big picture, what you have is heat flowing out of solid iron and cooling it down. So, you have to use the heat flow equation:...
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In a experiment it is observed that 252 J of heat must be absorbed to raise the temperature of 50.0 g of Ni(s) from 20.0 C to 31.4 C. How do you calculate the specific heat of Ni in both J/g °C and cal/g.C?
The equation to use is $Q=mcDeltaT$, where $Q$ is the energy in Joules, $m$ is the mass, $c$ is the specific heat, and $DeltaT$ is the change in temperature. $DeltaT=T_"final"-T_"initial"$...
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The specific heat of aluminum is 0.214 cal/g°c. What is the energy, in calories, necessary to raise the temperature of a 55.5 g piece of aluminum from 23.0 to 48.6°C?
The of aluminium tells you the amount of energy needed to increase the temperature of $"1 g"$ of aluminium by $1^@"C"$. $c_ "Al" = "0.214 cal g"^(-1)""^@"C"^(-1)$...
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If 8.40 kJ of heat is needed to raise the temperature of a sample of metal from 15 °C to 20 °C, how many kilojoules of heat will be required to raise the temperature of the same sample of metal from 25 °C to 40 °C?
The trick here is to realize that because the sample of metal has the same mass in both cases, you can say that $q_2 = (DeltaT_2)/(DeltaT_1) * q_1$...
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How much heat is required to raise the temperature of a 50.0 g block of iron by
$10.0^@"C"$ ? Specific heat of iron: $"0.449 J/g"""^@"C"$
The key to this problem is the of iron, which is said to be equal to $c_"iron" = "0.449 J g"^(-1)""^@"C"^(-1)$ As you know, the specific heat...
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Given the Following: heat of fusion of ice = 80.0 cal/g; specific heat of ice = 0.480 cal/g; and specific heat of water = 1.00 cal/g. Calculate the amount of heat required to melt 30.0 g of ice at 0 degrees celsius?
$H_2O(s) +DeltararrH_2O(l)$....... Note that BOTH the ice and water have a specified temperature of $0$ $""^@C$, and thus we assess the heat involved in the phase change, and thus we...
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The specific heat of ice is 0.492 cal/(g × °C). How many calories of heat are required to raise 100.0 g of ice from -20.0 °C to -0.5 °C?
And so we simply take the product... $"mass"xx"C"_"specific heat"xxDeltaT=100.0*gxxunderbrace(0.492*cal*g^-1*""^@C^-1)_"quoted specific heat"xx19.5*""^@C=+959.4*cal$....the positive sign indicates heat is ADDED to the system.
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A calorimeter contains 15 grams of water. The water's temperature increases by 10 C°. How much heat energy was added to the water? (Hint: water's specific heat is 1 cal/g°C)?
Unsurprisingly, the key to this problem is the hint. The thing to remember about a substance's is that it tells you the amount of energy needed in order...
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What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10°C? (Specific heat of aluminum = -0.21 cal/g*$"^@$C)?
Here, we're relating a few things: (1) the mass of the substance, (2) its , and (3) its temperature change with the equation, $q = mC_sDeltaT$ Before we start, that...
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How many calories are required to raise the temperature of a 35.0 g sample of iron from 25°C to 35°C? Iron has a specific heat of 0.108 cal/g°C?
The key to this problem lies in the value of the of iron. $c_"iron" = "0.108 cal"$ $color(blue)("g"^(-1))color(darkorange)(""^@"C"^(-1))$ This tells you that in order to increase...
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