Enter your answer in the provided box.   Acetylene burns in air according to the following equation:   C2H2(g) +  5   2  O2(g)  →  2 CO2(g) + H2O(g)   Δ H o   rxn  = −1255.8 kJ

At constant volume, the heat of combustion of a particular compound, compound A, is −3520.0 kJ/mol.−3520.0 kJ/mol. When 1.439 g1.439 g of compound A (molar mass =112.71 g/mol)=112.71 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.391 ∘C.6.391 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?

The combustion of propane (C3H8) produces 2220 kJ of energy per mole of propane consumed. What mass in grams of propane will be required to heat 55.0 gal of bathtub water from 25.0°C to 35.0°C if the process is 80.0% efficient? (1 gal = 3.785 L, 1 cal = 4.184 J, the density of water is 1.00 g/mL, the specific heat of water is 1.00 cal/(g°C)

If a 50.0g sample of Cu is heated to 180.00C and is placed in 100.0 ml of water in a calorimeter at 25.00C, what will the final temperature be for the system? Assume that all of the heat goes from the copper to the water. (None is lost to the surroundings or calorimeter.) dH20 =1.00g/ml C Cu = 0.385J/goC CH2O = 4.184 J/goC

Consider the hypothetical thermochemical equation 3 A + B → 2 C for which ΔH = 58.7 kJ/mol. If the reaction absorbs 345 kJ of heat, What quantity in moles of C would be produced?

2. Using Hess's Law, Calculate enthalpy change for: NO (g) + O₂ (g) → NO₂ (g) Given the following enthalpies of reaction ½ N₂ (g) + O₂(g) → NO₂(g) AH = + 33.8 kJ 12 N₂ (g) + 1/2O2 → NO (g) AH = -566.0 kJ

You add some of the white crystals to a small test tube filled with water. The water in the test tube was initially at room temperature (25˚C). Once the crystals were added and the tube was stirred, the temperature of the solution decreased to about 15˚C and all of the crystals dissolved. what is the change in enthalpy (∆H) for this process?

lodic Tabie The flame in a torch used to cut metal is produced by burning acetylene (C2H2) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 35.1 × 104 kJ of heat? g

Calculate the energy required to heat 0.40 kg of ammonia from 56.1 °C to 65.4 °C. Assume the specific heat capacity of 1 ammonia under these conditions is 4.70 J·g¯¹·K¯¹ Be sure your answer has the correct number of significant digits.

When a 1.0 g sample of a candy bar is combusted in a bomb calorimeter whose total heat capacity (including the water) is 5.0 kJ/°C, the temperature of the water increases by 6.0 °C. If the candy bar has a mass of 28 g, calculate the total number of Calories that it contains. (1 Calorie = 103 calories, and 1 calorie = 4.184 J). Give your answer to the nearest 100 Calories, but not in scientific notation. Type your answer.