Calculate the amount of heat in joules that 12.5 g of ethanol, C₂H₆O(l), would need to absorb to increase in temperature by 16.0^oC.

Calculate the amount of heat in joules that 56.8 g of aluminum, Al(s), would need to absorb to increase in temperature from 33^oC to 72^oC.

Calculate the amount of heat in joules that 56.8 g of copper, Cu(s), would need to absorb to increase in temperature from 33^oC to 72^oC.

What is the mass of a sample of gold that absorbs 650 J of energy and increases in temperature by 16^oC?

What is the mass of a sample of lead that absorbs 650 J of energy and increases in temperature by 16^oC?

A sample of iron increases in temperature from 100.0^oC to 275^oC by absorbing 5000.0 J. What is the mass of this sample of iron?

A sample of CO₂(g) increases in temperature from 50.0^oC to 75.0^oC by absorbing 4722 J. What is the mass of this sample of CO₂?

What is the temperature change when 175 g He absorbs 6505 J of energy?

What is the temperature change when 615 g silicon, Si(s), absorbs 4568 J of energy?

What is the final temperature of 72 g H2O at 20^oC, absorbs 24,100 J of energy?

You have a hot plate of green beans that are too hot to eat as they are at 95^oC. You place the plate in the freezer for a few minutes where the green beans lose 3500 J of heat. If the green beans have a mass of 45 g, what is the final temperature of the green beans? The specific heat of green beans is 1.96 J/g^oC.

Two pieces of lead each absorbed the same amount of energy. One piece of lead was 15.0 grams and the other piece of lead was 150.0 grams. Which piece of lead had a higher final temperature?

Two samples of mercury each absorbed 1600 J of energy. One of the samples of mercury had a mass 10 times greater than the other one. Which sample of mercury had a higher final temperature?

A 70.0 g piece of metal at 80.0 °C is placed in 100 g of water at 22.0 °C contained in a calorimeter. The metal and water come to the same temperature at 24.6 °C.

What is the specific heat of the metal?

A 40.5 g piece of metal at 100.0 °C is placed in 105 g of water at 20.0 °C contained in a calorimeter. The metal and water come to the same temperature at 22.76 °C.

What is the specific heat of the metal?

A 40.5 g piece of metal at 100.0 °C is placed in 105 g of water at 20.0 °C contained in a calorimeter. The metal and water come to the same temperature at 22.76 °C.

What is the temperature change of the water?

A 40.5 g piece of metal at 100.0 °C is placed in 105 g of water at 20.0 °C contained in a calorimeter. The metal and water come to the same temperature at 22.76 °C.

What is the temperature change of the metal?

A 40.5 g piece of metal at 100.0 °C is placed in 105 g of water at 20.0 °C contained in a calorimeter. The metal and water come to the same temperature at 22.76 °C.

How much energy in J did the water gain?

When 50.0 g of 0.200 M NaCl(aq) at 24.1 °C is added to 100.0 g of 0.100 M AgNO₃(aq) at 24.1 °C in a calorimeter, the temperature increases to 25.2 °C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g °C, calculate the approximate amount of heat in joules produced.

When 150.0 g of 0.200 M NaCl(aq) at 23.4 °C is added to 150.0 g of 0.100 M AgNO₃(aq) at 23.4 °C in a calorimeter, the temperature increases to 26.1 °C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g °C, calculate the approximate amount of heat in joules produced.

1. When 0.02 mols of AgNO₃ reacts with NaCl, 1.34 kJ of heat is released.

2. Calculate ΔH in kJ/mol of AgNO₃(aq) for the reaction:

3. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)

1. When 0.35 mols of N₂ reacts, 63.21 kJ of heat is absorbed.

2. Calculate ΔH in kJ/mol for the reaction:

3. N₂(g) + O₂(g) → 2 NO(g)

1. When 0.75 mols of O₂ is produced according to the following reaction, 147 kJ of heat is released.

2. Calculate ΔH in kJ/mol for the reaction:

3. 2 H₂O₂(l) → 2 H₂O(l) + O₂(g)

1. 2 H₂O(l) + O₂(g) → 2 H₂O₂(l) $$\Delta$$ H = + 196 kJ

2. When 2 moles of O₂ react according to the above thermochemical reaction, how much heat energy is absorbed?

1. 2 H₂O(l) + O₂(g) → 2 H₂O₂(l) $$\Delta$$ H = + 196 kJ

2. When 3.5 moles of H₂O react according to the above thermochemical reaction, how much heat energy is absorbed?

1. N₂(g)  +  3 H₂(g) → 2 NH₃(g) ΔH = -91.8 kJ

   When 2.5 moles of H₂ react according to the above thermochemical reaction, how much heat energy is released?

1. N₂(g)  +  3 H₂(g) → 2 NH₃(g) ΔH = -91.8 kJ

   When 2.5 moles of N₂ react according to the above thermochemical reaction, how much heat energy is released?

1. N₂(g)  +  3 H₂(g) → 2 NH₃(g) ΔH = -91.8 kJ

   When 1.75 moles of NH₃ is produced according to the above thermochemical reaction, how much heat energy is released?

1. Calculate ΔH° for the process

(i) Sb(s) + 5/2 Cl₂(g) → SbCl₅(s) ΔH° = ?

from the following information:

(ii) Sb(s) + 3/2 Cl₂(g) → SbCl₃(s) ΔH° = −314 kJ

(iii) SbCl₃(s) + Cl₂(g) → SbCl₅(s) ΔH° = −80 kJ

1. Calculate ΔH for the process 

(i) Hg₂Cl₂(s) ⟶ 2 Hg(l) + Cl₂(g) ΔH = ?

from the following information:

(ii) Hg(l) + Cl₂(g) ⟶ HgCl₂(s) ΔH = −224 kJ

(iii) Hg(l) + HgCl₂(s) ⟶ Hg₂Cl₂(s) ΔH = −41.2 kJ

1. Calculate ΔH° for the process 

(i) Co₃O₄(s) ⟶ 3 Co(s) + 2 O₂(g) ΔH° = ?

from the following information:

(ii) Co(s) + ½ O₂(g) ⟶ CoO(s) ΔH° = −237.9kJ

(iii) 3 CoO(s) + ½ O₂(g) ⟶ Co₃O₄(s) ΔH° = −177.5kJ

When 2.0 moles of carbon monoxide combusts according to the reaction on this chart, how many kJ of energy is released?

When 2.5 moles of methane combusts according to the reaction on this chart, how many kJ of energy is released?

When 1.75 moles of acetylene combusts according to the reaction on this chart, how many kJ of energy is released?

When 3.84 moles of ethanol combusts according to the reaction on this chart, how many kJ of energy is released?

When 7.5 moles of isooctane combusts according to the reaction on this chart, how many kJ of energy is released?

When a sample of sulfur combusts according to the reaction written on this chart, 742 kJ of energy was released. How many moles of sulfur combusted?

When a sample of methane combusts according to the reaction written on this chart, 1648 kJ of energy is released. How many moles of methane combusted?

When a sample of methanol combusts according to the reaction written on this chart, 3478 kJ of energy is released. How many moles of methanol combusted?

When a sample of isooctane combusts according to the reaction written on this chart, 25,830 kJ of energy is released. How many moles of isooctane combusted?

Convert 3.95 J to calories

Convert 9.17 J to calories

Convert 16.8 calories to joules

Convert 38,180 J to kJ

Convert 17,298 J to kJ

Convert 43.5 kJ to J

Convert 216 kJ to J