When 3.0 grams of H2 is reacted with excess C at constant pressure, the reaction forms CH4 and releases 51.9 kJ of heat. C(s) + 2 H2(g) --> CH4(g) What is the enthalpy of the reaction in kJ/mol of CH4?

It is recommended that the average daily intake of glucose for humans is not to exceed 32.5 g of glucose (C6H12O6). The balanced chemical equation for the combustion of glucose is shown below. C6H12O6(aq) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O (1) AH rxn= -1273.3 kJ/mol How much heat is released when 55.5 g of oxygen are combusted with glucose as shown in the reaction. above? Use the provided Periodic Table for any calculations involving elements. Report your answer to a single decimal place and report proper units with your answer.

In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6 C. After the reaction, the final temperature is 31.3 C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.

At constant volume, the heat of combustion of a particular compound, compound A, is −3046.0 kJ/mol.−3046.0 kJ/mol. When 1.753 g1.753 g of compound A (molar mass =112.07 g/mol)=112.07 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.475 ∘C.6.475 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?     Suppose a 3.771 g3.771 g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 25.65 ∘C25.65 ∘C to 29.76 ∘C.29.76 ∘C. What is the heat of combustion per gram of compound B?

A 1.615-g sample of benzoic acid, C7H6O2 (122.12 g/mol) was burned in a bomb calorimeter with excessoxygen. The temperature of the calorimeter and the water before combustion was 17.49 °C; after combustionthe calorimeter and the water had a temperature of 27.28 °C. The calorimeter had a heat capacity of 832 J/K,and contained 0.837 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of benzoicacid.

A 3.59°C increase in temperature occurs when a 0.232 g sample of benzoic acid (C7H6O2) is combusted in a bomb calorimeter. A 1.81 °C increase in temperature occurs when a 0.303 g sample of citric acid (C6H8O7) is combusted in the same bomb calorimeter. The heat of combustion of benzoic acid is -26.37 kJ/g. What is the molar heat of combustion of citric acid? Reminder: Any heats of combustion will be negative since these are exothermic reactions.

What quantity of heat (in kJ) will be released if 0.1673 mol of NH³ are mixed with 0.200 mol of O: in the following chemical reaction? 4 NH (g) + O: (g) → 2 N₂H4 (g) + 2 H₂O (g) AH = -286 kJ/mol

When 3.0 grams of H2 is reacted with excess C at constant pressure, the reaction forms CH4 and releases 58.6 kJ of heat. C(s) + 2 H2(g) --> CH4(g) What is the enthalpy of the reaction in kJ/mol of CH4? Enter your answer numerically and in terms of kJ/mol.