Identify each as either endothermic or exothermic 

a. Formation of morning dew on plants

b. Burning wood

c. Formation of dry ice fog

Predict whether the following reactions will be exothermic or endothermic.

a. N₂(g) + 3 H₂(g) → 2 NH₃(g)

b. S(g) + O₂(g) → SO₂(g)

c. CaO₃(s) → CaO(s) + CO₂(g)

d. 2 H₂O(g) → 2 H₂(g) + O₂(g)

e. 2 F(g) → F₂(g)

Tungsten metal has a high strength-to-weight ratio and is known to withstand high temperatures, making it viable in military and marine industries. The molar heat capacity of tungsten is 24.3 J/mol ºC. Calculate the specific heat capacity of tungsten.

Consider two metal blocks, each weighing 250.0 g. One block is made of titanium and the other is made of platinum. Each block absorbed  16.34 kJ of heat. Identify which of the two metal blocks will have a higher rise in temperature. The molar heat capacities of Ti and Pt are 25.03 J/mol-°C and 25.86 J/mol-°C respectively.

Which substance would have the greatest temperature change upon absorbing 200.0 J of heat?

a) 5.0 g NH₃, C_NH3 = 4.700 J/g°C

b) 5.0 g Li, C_Li = 3.58 J/g°C

c) 5.0 g Fe, C_Fe = 0.412 J/g°C

d) 5.0 g H₂O, C_H2O = 4.181 J/g°C

e) 5.0 g Na, C_Na = 1.230 J/g°C

The complete combustion of a hydrocarbon produced 17.2 g of CO₂ and 2.45 g of H₂O. The heat given off was 463 kJ.  Determine the mass of the substance combusted.

A 1.00 kg block of nickel metal was heated to 98.0 °C. It was dropped in a coffee cup calorimeter containing 350.0 g of water at 25.8 °C. The temperature inside the cup became 41.3 °C. If the heat loss from the metal was all absorbed by the water, what would be the final temperature of the system?

The heat of dissolution is the heat evolved or absorbed when a solid dissolves in water, and can be determined using a coffee cup calorimeter.

A student finds that when 5.00 g of CuSO₄(s) is dissolved in 120 g of water, the temperature of the solution increases from 23 to 28.9 °C. In a separate experiment, the heat capacity of the calorimeter was determined to be 1.65 J/°C. Calculate the heat of dissolution of CuSO₄(s) in kJ/mol based on these findings. Assume the specific heat of the solution is equal to the specific heat of water.

A 5.60 g sample of Phenalene (C₁₃H₁₀) is burned in a bomb calorimeter and the temperature increases from 21.52 to 41.21 °C. Calculate the total heat capacity of the calorimeter given that the heat of combustion of phenalene is -42.35 kJ/g. 

A 3.50 g sample of Ribose (C₅H₁₀O₅) is burned in a bomb calorimeter and the temperature increases from 20.30 to 30.50 °C. Calculate the total heat capacity of the calorimeter given that the heat of combustion of Ribose (C₅H₁₀O₅) is -15.62 kJ/g. Also, calculate the temperature change if half of the initial sample of ribose was used.

A 4.50 g sample of naphthalene (C₁₀H₈) is burned in a bomb calorimeter and the temperature increases from 20.00 to 50.37°C

Calculate the heat of combustion per gram of naphthalene and per mole of naphthalene given that the total heat capacity of the calorimeter is 5.960 kJ/°C. 

Consider the two substances M and N. Substance M has a mass of 5.16 g and is initially at 18.6°C. Substance N has a mass of 22.3 g and is initially at 56.4°C. The two substances come into contact with each other and reach thermal equilibrium. The final temperature of both substances is 49.7°C. Given that the specific heat capacity of substance N is 2.34 J/g•°C, calculate the specific heat capacity of substance M.

2 crates of beer were packed in coolers and were brought on a camping trip. Each crate contains 12 bottles of beer that can fit into 1 cooler (2 coolers total). 

The night before the trip, a crate of beer bottles was refrigerated and the other crate was stocked at room temperature due to limited space in the fridge. 

In the morning, the bottles were packed in the cooler together with gel ice packs. Each cooler had 10 ice packs each and 12 beer bottles. Cooler 1 had the refrigerated beer while cooler 2 had the room temperature beer. 

Explain why the ice packs in cooler 1 were still solid while they were all melted in cooler 2 by the time the camping site was reached,