A bomb calorimeter can be used to measure the enthalpy of reaction for combustions, such as the combustion of diborane represented by the following balanced equation: B2​H6​(g)+3O2​(g)B2​O3​(s)+3H2​O(g) ΔHcombustion for this process is –1958 kJ/mol Assume that 0.251 g of diborane is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.854 kJ/°C at 16.31°C. What is the final temperature of the calorimeter?

According to the following thermochemical equation, what mass of C3H18 (in g) must react in order to produce 345 kJ of energy? Assume excess O2. The molar mass of octane (C3H18 ) is 114.33 g/mol. 2 C3H18 + 25 O2 - 16 CO2 + 18 H2O AH°rxn = -11018 kJ Units don't need to be typed in the answer. Answer:

A scientist measures the standard enthalpy change for the following reaction to be -737.2 kJ : 2Co(g) + 2 NO(g)2CO2(g) + N2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol.

When N2(g) reacts with H2(g) to form NH3(g) , 92.2 kJ of energy are evolved for each mole of N2(g) that reacts.Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation

A bomb calorimeter can be used to measure the enthalpy of reaction for combustions, such as the combustion of diborane represented by the following balanced equation:B2​H6​(g)+3O2​(g)➔B2​O3​(s)+3H2​O(g)ΔHcombustion for this process is –1958 kJ/mol. Assume that 0.411 g of diborane is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.854 kJ/°C at 22.61°C. What is the final temperature of the calorimeter? The answer is not 18.922°C

The balanced thermochemical equation for the combustion of exactly one mole of propane is: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O(l) ΔH = -2220 kJ/mol What is the enthalpy change for the reaction: 1.5 CO2 (g) + 2 H2O(l)  → 0.5 C3H8 (g) + 2.5 O2 (g) ΔH = ?

A scientist measures the standard enthalpy change for the following reaction to be -912.5 kJ:2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is  kJ/mol.

When methanol, CH3OH,CH3OH, is burned in the presence of oxygen gas, O2,O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJCH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJ How much methanol, in grams, must be burned to produce 639 kJ639 kJ of heat?