Convert 440 Calories (nutritional) to joules.

The SI unit of heat and energy is the __________.

A baked potato contains 245 Calories. Calculate the energy in joules.

What is the equation for calculating heat?

Based on the figure, which of the following statements is true?

The formation of AlCl₃ began at 0.0^oC.

The final temperature of the reactants was -704^oC.

The final temperature of the products was -704^oC.

The formation of AlCl₃ releases energy.

The _____ law of thermodynamics states that energy is neither created nor destroyed.

first

second

third

fourth

When your body breaks down sugars and fats to form carbon dioxide and water, these exothermic reactions generate __________.

calories

joules

heat

watts

One calorie equals __________ joules.

One joule is the equivalent of __________ calories.

How much heat is evolved from 54.0 g glucose (C₆H₁₂O₆), according to the equation for calculating heat?

$$C_6H_{12}O_6\ +\ 6O_2\ \rightarrow\ 6H_2O\ +\ 6CO_2\ \ \ \Delta H\ =\ -2808\ kJ$$

What is the specific heat of a metal that weighs 25 g and absorbs 110 J when the temperature is increased by 60°C?

The specific heat of water is 4.184 J/(g°C). How much heat is absorbed by 30 g of water when its temperature is increased from 20.0°C to 75.0°C?

Calculate the amount of heat absorbed by 12.0 g of water when its temperature is raised from 21.0°C to 52.0°C. The specific heat of water is 4.18 J/(g°C).

An endothermic reaction absorbs 540 J. How many calories are absorbed in the reaction?

Calculate the heat required to melt 78.0 g of solid ethanol C₂H₅OH given that the molar enthalpy of fusion is 4.9 kJ/mol. The molar mass of ethanol is 46 g/mol.

Use standard enthalpies of formation to calculate the enthalpy change for the following reaction:

$$C_2H_4\ \left(g\right)\ +\ 3O_2\ \left(g\right)\ \rightarrow\ 2CO_2\ \left(g\right)\ +2H_2O\ \left(g\right)$$

C₂H₄(g): +52.26 kJ/mol

CO₂(g): –393.509 kJ/mol

H₂O(g): –241.818 kJ/mol

Calculate the amount of heat released in the complete combustion of 8.17 g of Al to form Al₂O₃(s) at 25⁰C and 1 atm.

ΔH_f^o for Al₂O₃(s) = -1680 kJ/mol.

$$4Al\ \left(s\right)\ +\ 3O_2\ \left(g\right)\ \rightarrow\ 2Al_2O_3\ \left(s\right)$$

Calculate ΔH for the reaction below.

$$4HCl\ \left(g\right)\ +\ O_2\ \left(g\right)\ \rightarrow\ 2Cl_2\ \left(g\right)+\ 2H_2O\ \left(g\right)\ \ \ \ \Delta H\ =\ ?\ kJ$$

$$H_2\ \left(g\right)\ +\ Cl_2\ \left(g\right)\ \rightarrow\ 2HCl\ \left(g\right)\ \ \ \ \Delta H\ =\ -185\ kJ$$ $$2H_2\ \left(g\right)\ +\ O_2\ \left(g\right)\ \rightarrow\ 2H_2O\ \left(g\right)\ \ \ \Delta H\ =\ -483.7\ kJ$$

Copper metal has a specific heat of 0.385 J/g • ⁰C. Calculate the amount of heat required to raise the temperature of 22.8 g of copper from 20.0⁰C to 875⁰C.