Elemental iron is used in heat packs and the reaction can be represented as: 4 Fe(s) +3 O2(g) → 2 Fe2O3 (s) AH=-1652 kJ How much heat is released when 8.5 g of iron react with excess O2? 62.9 kJ 194 kJ 251 kJ 1006 kJ

Energy for recycling Cu: ________ kJ

The heat of reaction for the reaction A + 2B → 2C is 900. kJ.The heat of reaction for the reaction B + D → C is 150. kJ.Using Hess's Law, calculate the heat of reaction for the reaction A → 2D.

In the following reaction, how much heat (in kJ) is released when 6.35 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol

In the following reaction, what is the quantity of heat (in kJ) released when 3.91 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO₂ (g) + 2 H₂O(g) AH° = -802 kJ/mol -

The reaction between sodium metal and chlorine gas produces 822 kJ of heat energy for every chlorine molecule consumed [2 Na(s) + Cl2(g) → 2 NaCl(s)]. How much heat is released (in kJ) if 1.569 g of Na are consumed in the reaction?

In the following reaction, how many moles of CH;OH are required to produce -2191 kJ of heat? 2 CH;OH (I) + 3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH° = -1280. kJ mol 1 3 4 6. C 7 8 9. + +/- x 100

A 837837 g copper pan is removed from the stove at a temperature of 150 °C. It is then stacked on top of a 787787 g aluminum sheet at room temperature, 25 °C. The specific heat capacity for copper is 0.387 Jg·KJg·K and that for aluminum is 0.904 Jg·KJg·K. Assume no heat is gained or lost to the surroundings.   What is the final temperature (?fTf) of the two objects after thermal equilibrium is reached?

How many kilojoules of heat are produced when 6.04 mol of Al react?     2Al(s) + Fe2O3(s) →  2Fe(s) + Al2O3(s)      heat of reaction = –851.5 kJ

Calcium carbonate, CaCO3 is used as a calcium supplement. When it is heated, it decomposes to form calcium oxide and carbon dioxide. The energy used for the decomposition of calcium carbonate is y kJ. The balanced chemical equation for the reaction is a. CaCO3(s) → CaO(s) + CO2(g)                    ΔH = +y kJ b. 2CaCO3 (s) → 2CaO(s) + 2C(s) + 2O2(g)    ΔH = +2y kJ c. CaCO3(s) → CaO(s) + CO2(g)                    ΔH = –y kJ d. 2CaCO3(s) → 2CaO + 2CO2(g)                  ΔH = –2y kJ e. none of the above