- 1(current)
Q. No.The heat capacity of a system is defined as:
| 1. | The heat required to raise the temperature of the system by 1 degree Celsius. |
| 2. | The heat released when the system undergoes a chemical reaction. |
| 3. | The heat absorbed when the system undergoes a chemical reaction. |
| 4. | The heat required to raise the temperature of the system by 1 Kelvin. |
Subtopic: Calorimetry |
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Which of the following statements about exothermic reactions is true?
1. They absorb heat from the surroundings
2. They have a positive change in enthalpy \((\Delta \mathrm{H})\)
3. They release heat to the surroundings
4. They occur spontaneously at low temperatures
1. They absorb heat from the surroundings
2. They have a positive change in enthalpy \((\Delta \mathrm{H})\)
3. They release heat to the surroundings
4. They occur spontaneously at low temperatures
Subtopic: Calorimetry |
80%
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The heat of vaporization is the heat:
1. Absorbed when a solid changes to a liquid.
2. Released when a gas changes to a liquid.
3. Absorbed when a liquid changes to a gas.
4. Released when a liquid changes to a solid
1. Absorbed when a solid changes to a liquid.
2. Released when a gas changes to a liquid.
3. Absorbed when a liquid changes to a gas.
4. Released when a liquid changes to a solid
Subtopic: Calorimetry |
81%
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Hess's law states that:
| 1. | The heat evolved in a given process is equal to the heat absorbed in the reverse process. |
| 2. | The heat evolved or absorbed in a chemical process is the same regardless of the pathway taken. |
| 3. | The heat of reaction depends on the temperature of the reaction. |
| 4. | The heat of reaction is directly proportional to the concentration of the reactants. |
Subtopic: Calorimetry |
71%
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What is the heat of neutralization for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH)?
1. -57.32 kJ/mol
2. -13.7 kJ/mol
3. -57.32 kJ/g
4. -13.7 kJ/g
1. -57.32 kJ/mol
2. -13.7 kJ/mol
3. -57.32 kJ/g
4. -13.7 kJ/g
Subtopic: Calorimetry |
76%
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Subtopic: Calorimetry |
84%
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