Consider the following reaction: CH4 (g) + 2O2 (g) --> CO2 (g) + 2H2O (l)  and  deltaH = -891 kJ. Calculate the enthalpy change for each of the following cases: a. 1.00 g methane is burned in excess oxygen. b. 1.00 * 103 L methane gas at 740. torr and 25°C are burned in excess oxygen

10. Calculate the standard enthalpy of formation of N₂O5 from the following data: kJ mol kJ 2NO(g) + O₂(g) →2NO₂(g) 4NO2(g) + O₂(g)→2N205(g) N₂(g) + O₂(g) →2NO(g) 4,H☺ = -114.1 = -110.2- 'mol kJ mol AH AH = + 180.5,

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…

Consider the following reaction: CH4 (9) + 20, (g) → CO2(g) + 2H,0(1) AH=-891 kJ a. Calculate the enthalpy change if 2.59 g methane is burned in excess oxygen. Enthalpy change = kJ b. Calculate the enthalpy change if 3.04 × 10° L methane gas at 737 torr and 25°C is burned in excess oxygen. Enthalpy change = kJ

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 8.000 g tablet of benzoic acid (C6H₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 10.00 °C to 47.00 °C over a time of 5.8 minutes. olo Next, 5.940 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 10.00 °C to 55.55 °C. Ar chemical reaction Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: "bomb" A "bomb" calorimeter. C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(g) 4 Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…

Consider the following chemical reaction: C2H6O(l) + O2(g) -----------> CO2(g) + H2O(g)  0.8100 g C2H6O(l) is burned in bomb calorimeter.   The initial temperature is 22.000 oC and the temperature rises to 28.200 oC.     Calculate the heat of reaction at constant pressure  at 22.0 oC in kJ/mole C2H6O      The heat capacity of calorimeter is 10.50 kJ/ oC. C= 12.01 g/mole, H = 1.008 g/mole,  O = 16.00 g/mole

Cl2 (g) + H2 (g) → 2 HCl (g) ΔH0rxn = ‒184.6 kJ 8. What is ΔH0rxn when 4.50 mol HCl (g) forms? (Slides 17 – 18: Stoichiometry of Thermochem. Eq.) Group of answer choices A.‒831 kJ B.‒415 kJ C.‒207 kJ D.831 kJ E.415 kJ

Acetylene (CH2) is commonly used as a fuel for welding. a) Write a balanced chemical equation that describes the combustion of acetylene. b) Calculate AHrn for the combustion of 1 mole of acetylene. c) A steel MC cylinder can contain 310 grams of acetylene. Calculate the heat released by the combustion of the acetylene in 1 steel MC cylinder. d) How much water can you warm from 20 °C to 90 °C using 310 grams of acetylene. e) How much ice can you melt at 0 °C using 310 grams of acetylene.

When 56.8 of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0 degrees Celsius, 60.1 kj of heat is released at constant pressure. What is the change in enthalpy at standard condition for the reaction (Please type answer no write by hend)

A 23.0 gram sample of an alloy was heated to 100.00 °C and dropped into a beaker containing 92 grams of water at 25.84 °C. The temperature of the water rose to a final temperature of 27.84 °C. Neglecting heat losses to the room and the heat capacity of the beaker itself, what is the specific heat of the alloy in /g°C? а. 2.16 ОБ. 0.464 O c. 0.232 O d. 4.32