Here's a problem for you to solve:What is the enthalpy change (∆H) for the combustion of methane (CH4) to form carbon dioxide (CO2) and water (H2O) based on the following information?CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) ∆H = -890.4 kJ/molYou have a sample of methane and you want to determine the heat released or absorbed during combustion. How much heat is produced when you burn 5.00 grams of methane (CH4) at a constant pressure of 1 atm, assuming that the products are carbon dioxide (CO2) and water (H2O) and that the heat capacity of the calorimeter is negligible?

Question

Here's a problem for you to solve:What is the enthalpy change (∆H) for the combustion of methane (CH4) to form carbon dioxide (CO2) and water (H2O) based on the following information?

Answer 1

To determine the heat produced when burning 5.00 grams of methane, we first need to convert the mass of methane to moles. The molar mass of methane  CH4  is 12.01 g/mol  for carbon  + 4 * 1.01 g/mol  for hydrogen  = 16.05 g/mol.Now, we can convert the mass of methane to moles:5.00 g CH4 *  1 mol CH4 / 16.05 g CH4  = 0.3115 mol CH4The enthalpy change  H  for the combustion of methane is given as -890.4 kJ/mol. This means that 890.4 kJ of heat is released when 1 mol of methane is burned. To find the heat produced when burning 0.3115 mol of methane, we can use the following equation:Heat produced  q  = moles of CH4 * H per mole of CH4q = 0.3115 mol CH4 *  -890.4 kJ/mol CH4  = -277.4 kJTherefore, 277.4 kJ of heat is produced when burning 5.00 grams of methane at a constant pressure of 1 atm.