C2H4 (g) + 3 02 (g)2 CO2 (g) + 2 H20 (e) Standard enthalpies of formation of CO2 (g) and H20 (e) are 4.00 x 102 k/mol and 2.90 x 102 k/mol, respectively. When 6.72 L CO2 (g) at STP is formed via the given reaction, 210 kj of heat is released. Which of the following statements is/are true for this reaction? I. When this reaction is carried out at constant pressure and temperature, work is done on the reacting system by the surroundings. II. The standard enthalpy of formation of C3H4 (g) is- 2780 kj/mol. III. 145 k) of heat is released when 9.01 g H20 (e) is formed via the given equation.

1. The formation of gaseous phosphorus trichloride is shown below:   P4 (g) + 6 Cl2 (g) → 4 PCl3 (g)     ΔH = -1207 kJ/mol   If 4.30 kJ of heat are released as the formation reaction above proceeds, how many milliliters of gaseous phosphorus trichloride, measured at 35°C and 712 torr, will be produced?

How many moles of H₂ are required to give off -9551 kJ of heat in the following reaction? N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol

11. A car has been fitted with an internal combustion engine that uses ethane as a fuel, which undergoes the following reaction when combusted: 2C2H6(g) + 702(g) → 4CO2(g) + 6H2O(g). Ethane (C2H6) has a molecular weight of 30.1 g/mol and a heat of reaction of -2,855.4 kJ/mol at 25°C. What is the AS° for this reaction at 25°C?

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?

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

Apps MyUSU Outlook Canvas Labflow OneNote 101 Chem101 Tophat U USU Tutoring Question 9 of 19 What quantity of heat (in kJ) is absorbed in the process of making 0.957 mol of CF from the following reaction? C (s) + 2 F, (g) → CF, (g) AH° = 141.3 kJ/mol 4. %3D

Determine the amount of heat (in kJ) given off when 2.56 g of NO2 is produced according to the following equation: 2NO(g) + O2(g) → 2NO2(g)          ΔH = −114.6 kJ/mol Group of answer choices 3.19 kJ 5.56 kJ 6.38 kJ 1.14 kJ 114.6 kJ

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