Q. No.\(100\) g water at \(20^\circ\text{C}\) is mixed with \(300\) g water at \(100^\circ\text{C}\) in a calorimeter. The mixture is now mixed again with \(400\) g water at \(10^\circ\text{C}.\) The final temperature of the mixture, assuming no loss of heat, is:
1. \(16^\circ\text{C}\)
2. \(30^\circ\text{C}\)
3. \(40^\circ\text{C}\)
4. \(45^\circ\text{C}\)
Subtopic: Â Calorimetry |
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A piece of alloy of mass \(250~\text{g}\) (specific heat capacity \(=0.1 \times\) that of water) is placed in a furnace and then put into a calorimeter containing \(240~\text{g}\) of water at \(20^\circ\text{C}.\) The water equivalent of the calorimeter is \(10~\text{g}\). The final temperature of the mixture is \(50^\circ\text{C}.\) The temperature of the furnace is (nearly):
| 1. | \(250^\circ\text{C}\) | 2. | \(350^\circ\text{C}\) |
| 3. | \(600^\circ\text{C}\) | 4. | \(800^\circ\text{C}\) |
Subtopic: Â Calorimetry |
 68%
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Two liquids flow through a heat exchanger and exchange heat energy.
The first liquid has a mass flow rate \(\left(\dfrac{dm}{dt}\right)=r_1,\) and its temperature rises by \(\Delta\theta_1.\) For the second liquid, the flow rate \(\left(\dfrac{dm}{dt}\right)=r_2,\) and the temperature fall is \(\Delta\theta_2.\) The ratio of their specific heat capacities is:
The first liquid has a mass flow rate \(\left(\dfrac{dm}{dt}\right)=r_1,\) and its temperature rises by \(\Delta\theta_1.\) For the second liquid, the flow rate \(\left(\dfrac{dm}{dt}\right)=r_2,\) and the temperature fall is \(\Delta\theta_2.\) The ratio of their specific heat capacities is:
| 1. | \(\dfrac{\Delta\theta_1}{\Delta\theta_2}\) | 2. | \(\dfrac{r_1}{r_2}\) |
| 3. | \(\dfrac{r_2\Delta\theta_2}{r_1\Delta\theta_1}\) | 4. | \(\dfrac{r_2\Delta\theta_1}{r_1\Delta\theta_2}\) |
Subtopic: Â Calorimetry |
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A piece of iron of water equivalent \(10 \) g is taken from a furnace and put into a calorimeter containing \(100\) g of water at an initial temperature of \(20^{\circ} \text{C}.\) The final temperature of the system is observed to be \(80^{\circ} \text{C}.\) Ignore the thermal capacity of the calorimeter and any loss of heat. The temperature of the furnace is:
1. \(600^{\circ} \text{C}\)
2. \(620^{\circ} \text{C}\)
3. \(680^{\circ} \text{C}\)
4. \(520^{\circ} \text{C}\)
1. \(600^{\circ} \text{C}\)
2. \(620^{\circ} \text{C}\)
3. \(680^{\circ} \text{C}\)
4. \(520^{\circ} \text{C}\)
Subtopic: Â Calorimetry |
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A calorimeter contains \(270\) g of ice at \(0^\circ\)C (specific latent heat \(80\) cal/g). Steam (specific latent heat \(540\) cal/g) at \(100^\circ\)C is continuously passed through it, and the excess steam is allowed to escape. Assume negligible loss of heat to the surroundings, except due to excess steam being allowed to escape. Also, ignore the heat capacity of the calorimeter. The final mass of water in the calorimeter is:
1. \(40\) g
2. \(90\) g
3. \(310\) g
4. \(360\) g
1. \(40\) g
2. \(90\) g
3. \(310\) g
4. \(360\) g
Subtopic: Â Calorimetry |
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\(200\) g of water at \(20^\circ\)C and \(300\) g of water at \(70^\circ\)C are mixed in a calorimeter of negligible heat capacity. Assume no loss of heat. The final temperature is:
1. \(40^\circ\)C
2. \(50^\circ\)C
3. \(60^\circ\)C
4. \(45^\circ\)C
1. \(40^\circ\)C
2. \(50^\circ\)C
3. \(60^\circ\)C
4. \(45^\circ\)C
Subtopic: Â Calorimetry |
 85%
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The SI unit of thermal capacity per unit volume is:
| 1. | joule/m3 | 2. | joule/kelvin |
| 3. | joule/kg-m3 | 4. | joule/kelvin-m3 |
Subtopic: Â Calorimetry |
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The specific heat capacity of a solid \(A\) is identical to that of another solid \(B\) at \(0^\circ\text C.\) The specific heat capacity of the solid \(A\) increases linearly by \(10\%\) from \(0^\circ\text C\) to \(100^\circ\text C;\) while that of solid \(B\) remains constant. If \(Q_A\) amount of heat is required to raise the temperature of solid \(A\) from \(0^\circ\text C\) to \(100^\circ\text C\) and \(Q_B\) be the heat required to raise the same mass of solid \(B\) from \(0^\circ\text C\) to \(100^\circ\text C,\) then,
| 1. | \(Q_A=1.1Q_B\) |
| 2. | \(Q_A>1.1Q_B\) |
| 3. | \(Q_A<1.1Q_B~\text{but}~Q_A>Q_B\) |
| 4. | \(Q_A=Q_B \) |
Subtopic: Â Calorimetry |
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A hot \(100~\text g\text-\)iron nail is dropped into a bucket of water at \(20^\circ\text C\) (initially) and the equilibrium temperature of the system is found to be \(21^\circ\text C.\) The mass of the water is \(5~\text{kg}.\) The specific heat capacity of iron is \(0.1~\text{cal g}^{-1}~^\circ\text C^{-1}.\) The temperature of the iron nail was, nearly:
1. \(500^\circ\text C\)
2. \(5000^\circ\text C\)
3. \(2500^\circ\text C\)
4. \(50^\circ\text C\)
1. \(500^\circ\text C\)
2. \(5000^\circ\text C\)
3. \(2500^\circ\text C\)
4. \(50^\circ\text C\)
Subtopic: Â Calorimetry |
 73%
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A calorimeter contains \(100~\text g\) water, and its initial temperature is \(50^\circ\text C,\) as measured by a sensitive thermometer. \(100~\text g\) of another liquid \(B,\) having half the specific heat of water, is added to it and the system is allowed to come to equilibrium. Assume no loss of heat in the process and ignore the thermal capacity of the calorimeter. The final temperature is found to be \(50^\circ\text C.\) The initial temperature, of the liquid \(B,\) is:
1. \(25^\circ\text C\)
2. \(50^\circ\text C\)
3. \(100^\circ\text C\)
4. \(75^\circ\text C\)
1. \(25^\circ\text C\)
2. \(50^\circ\text C\)
3. \(100^\circ\text C\)
4. \(75^\circ\text C\)
Subtopic: Â Calorimetry |
 74%
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