g piece of molybdenum, initially at 100.0°C, is dropped into a coffee-cup calorimeter containing 244 g of water at 10.0°C. When the system comes to thermal equilibrium, the temperature is 15.3°C. The specific heat of water is 4.184 J/(°C g). a. What is the specific heat of molybdenum? b. The specific heat of iron is 0.45 J/(°C g). I the same mass of iron at the same initial temperature had been dropped in the water, would the temperature of the water have raised more or less? (No calculations needed, just reasoning). 2.

g piece of molybdenum, initially at 100.0°C, is dropped into a coffee-cup calorimeter containing 244 g of water at 10.0°C. When the system comes to thermal equilibrium, the temperature is 15.3°C. The specific heat of water is 4.184 J/(°C g). a. What is the specific heat of molybdenum? b. The specific heat of iron is 0.45 J/(°C g). I the same mass of iron at the same initial temperature had been dropped in the water, would the temperature of the water have raised more or less? (No calculations needed, just reasoning). 2.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

2. A 237 g piece of molybdenum, initially at 100.0°C, is dropped into a coffee-cup calorimeter
containing 244 g of water at 10.0°C. When the system comes to thermal equilibrium, the
temperature is 15.3°C. The specific heat of water is 4.184 J/(°C g).
a. What is the specific heat of molybdenum?
b. The specific heat of iron is 0.45 J/(°C g). IK the same mass of iron at the same initial
temperature had been dropped in the water, would the temperature of the water
have raised more or less? (No calculations needed, just reasoning).

3. Given the AHxn in kJ/mol in square brackets for the following reactions:
C,H,0(1) +30,(g) → 2C0,(g)+ 3H,0(1)
C2H40(1) +5/202(g) →
Calculate the standard enthalpy of reaction for the following reaction in kJ:
[-685.5]
2C02(g) + 2H20(1)
[-583.5]
2C2H,0(1) + 2H20(1) → 2C,H,0(1) + 02(g)
4. Given the following AH in kJ/mol: HF(g) – 273.3;
H,0(1) – 285.8;
H20(g) – 241.8
Calculate the standard enthalpy of reaction for the following reaction:
2F2(g) + 2H,0(1) →
4HF(g) + 02(g)
Is the reaction endothermic or exothermic?

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