Select the single best answer. Consider the steps in coal gasification: C(coal) + H₂O(g) → CO(g) + H2(g) CO(g) + H₂O(g) → CO2(g) + H2(g) CO(g) + 3H2(g) → CH4(g) + H₂O(g) AH°rxn = 129.7 kJ AH rxn=-41 kJ AH°rxn=-206 kJ Identify the overall reaction for the production of methane, CH4.

Gaseous nitrosyl chloride (NOCl) is injected in a 1.0-L container where it starts decomposing irreversibly. 2NOCl(g) → 2NO(g) + Cl2(g) The container is insulated (no heat exchange with its surroundings) and has a movable part that allows one to change its volume. Before the reaction is over, the container’s volume is abruptly increased to 1.5 L. Use collision theory to explain how this will affect the rate at which NOCl decomposes

given the following reaction (see image) the enthalpy of the reaction of the nitrogen to produce nitic oxide is

2) Carbon dioxide can react with water to form carbonic acid - an important buffer in the blood. CO2(aq) + H2O) → H2CO3(aq) Calculate the AH°pm of this reaction. Is it exothermic or endothermic? Ixn

Octane (112.224 g/mol) undergoes combustion to form carbon dioxide gas and water vapor: 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g) ΔH°rxn = -1.01 x 105 kJ Given that the density of octane is 0.703 g/mL, what volume of octane must undergo combustion to produce 524 kJ of heat?

An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas.  In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g); ∆H = -1124 kJ.  The density of sulfur dioxide at 25 °C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/mol °C. a) How much heat would be evolved in producing 1.00 L of SO2 at 25 °C and 1.00 atm?  b) Suppose heat from this reaction is used to heat 1.00 L of SO2 from 25 °C to 500 °C for its use in the next step of the process.  What percentage of the heat evolved is required for this?

When 145 mL of 0.212 M NaCl(aq) and 145 mL of 0.212 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.7°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 3.14 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction.

Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 4 CH3NO2 (1) + 3 O2 (g) →4 CO2 (g) + 6 H20 (1) + 2 N2 (g), AH°rxn = -2836 kJ If 1,409 kJ of heat are produced from the burning of nitromethane, how many grams of nitromethane were burned? Enter your numerical answer in units of grams.

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 8.60kg of water at 28.2°C. During the reaction 107.kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18 J·g^−1K^−1.   Round your answer to 3 significant digits.