Calculate AHrxn for the following reaction: C(s) +H20(g)→CO(g) +H2 (g) Use the following reactions and given AH values: C(s) + O2(g)→CO2(g), AH = -393.5 kJ 2C0(g) + O2(g)→2CO2(g), AH = -566.0 kJ 2H2 (g) + O2 (g)-2H2O(g), AH -483.6 kJ Express your answer using four significant figures.

Based on the following reactions: Rxn A: C{s) + O2(g) → CO2 (g) AH°C = -393.5 kJ/mole Rxn B: C3H18() + 25/2 O2lg) → 8CO2(g) + 9H2O) AH°C = -5461 kJ/mole Which reaction would produce more heat 10*A or B? 10*A would produce more heat B would produce more heat they would produce the same amount of heat

Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l)                     ΔH1HA(aq) → H+(aq) + A-(aq)                        ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l)        ΔH3Choose the equation that shows the correct relationship between their enthalpy changes.

Given the information below: 2C(s) + 2H20(g) CH4(g) + CO2(g) AH° = 35.3 kJ 2C(s) + 2H20(g) 2C0(g) + 2H2(g) AH° = 462.6 kJ -> CH4(g) + H20(g)→ CO(g) + 3H2(g) AH° = -61.2 kJ %3D Calculate the enthalpy of reaction for the reaction below (in kJ) Co(g) + H20(g) → CO2(g) + H2(g) -366,1 kJ -488.5kJ -436.7 kJ +488.5 kJ +436,7 kJ +366.1kJ O0 0 O OO

When a 4.25-g sample of solid sodium nitrate dissolves in 50.0 g of water in a coffee-cup calorimeter, the temperature drops from 28.78 °C to 24.00 °C. Thermometer Glass stirrer Cork stopper Two Styrofoam® cups nested together Reaction mixture in solution ▾ Part A What is AH (in kJ/mol NaNO3) for the dissolution of sodium nitrate: NaNO3(s) →Na+ (aq) + NO3(aq) Assume that the specific heat of the solution is the same as that of pure water (4.18 J/g. K). O 1.08 kJ/mol O 5.19 kJ/mol O 20.0 kJ/mol O 1.24 kJ/mol O 21.7 kJ/mol Submit Request Answer

Calculate the value of AH for the following reaction: 2 NO₂ (g) N₂O4 (g) → based on the formation reactions for each of the reaction components as shown below: N2 (g) + O2(g) →→→ NO₂ (g) AH = 33.2 kJ/mol N₂ (g) + 2O2 (g) →→→ N₂O4 (g) AH₂ = 11.1 kJ/mol AH: kJ/mol

Consider these reactions: Reaction 1: H2 (9)+ Cl2 (g) → 2HC1(g) AH = -184.6 kJ %3D Reaction 2: 20F2 (g) → 02 (g) + 2 F2 (g) AH = -49.4 kJ Reaction 3: N2 (9) + 202 (9) - → 2NO2 (9) AH = +66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H2) when 1,529.0 kJ of energy is released from the system. Answer: g (mass must be positive; round to nearest whole number)

How much energy in kJ is released in burning 1.63 mL of gasoline (assuming that all of it is octane with a density of 0.692 g/mL and a molar mass of 114.23 g/mol)   The equation for the combustion reaction is C8H18(ℓ) + 25/2O2(g) → 8CO2(g) + 9H2O(ℓ)   ΔHf° kJ/mol C8H18(ℓ): -250.3 O2(g): 0 CO2(g): -393.5 H2O(ℓ): -285.8   Round your answer to 2 decimal places.

Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)   3 C(s) + 4 H2(g) → C3H8(g)           ΔH = – 118.2 kJ C(s) + O2(g) → CO2(g)                   ΔH = – 62.4 kJ H2(g) + 1/2 O2(g) →  H2O(g)          ΔH = – 182.5 kJ

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