A hot piece of iron is dropped into a beaker containing colder water. Which of t

Question

A hot piece of iron is dropped into a beaker containing colder water. Which of the following statements are is/are CORRECT? 1. Energy is transferred as heat from the iron to the water. 2. Thermal equilibrium is attained when the iron and the water reach the same temperature. 3. Thermal energy from the iron is converted to electrostatic energy in the water. a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 1, 2 and 3 If 495 J is required to change the temperature of 12.7 g of sodium chloride from 275.0 K to 335.0 K, what is the specific heat capacity of sodium chloride? a. 0.866 J/g-K b. 2.60 J/g-K c. 0.650 J/g-K d. 1.15 J/g-k e 2.83 times 10^3 J/g-k If the same amount of energy in the form of heat is added to 5.00 g samples of each of the metals below, which metal will undergo the largest temperature change? a. Ag b. Al c. Cu d. Fe e. Hg How much energy (in kJ) is required to change the temperature of 325 g aluminum from 32 degree C to 815 degree C? The specific heat capacity of aluminum is 0.897 J/g middot K. a. 238 kJ b. 284 kJ c. 46.3 kJ d. 228 kJ e. 2.16 kJ

Explanation / Answer

1) when hot metal is dipped in cold water then

a) the energy is trasnfered from metal to water (the temperature of metal decreases and that of water increases)

b) the equilibrium is attained when they both reach to same temperature

c) the thermal energy of metal is converted to thermal energy of water.

So option 1 and 2 are correct

24) the specific heat capacity is the amount of heat required to raise the temperature of 1g of compound by one degree centigrade

the heat required by 12.7grams of NaCl = 495 Joules

so for one gram = 495 / 12.7 J = 38.97 Joules

The heat is required to raise the temperature from 275 to 335

the change in temperature = 335-275 = 60 K

so to increase temperature by 60 K the heat required by 1 gram =38.97 J

so the heat required to increase temperature by 1 K = 38.97 / 60 = 0.649 J / g K

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