Thermo chemical equation for standard enthalpy of formation

Question

Assignment:

Question 1. Ca(s) + 2H₂0(l) →  Ca(OH)₂(OH)₂(aq) + H₂(g)

75.0g of Ca(AW = 40.08) are reacted with 40.0 H₂0 (MW = 18.02) according to the above equation if 30.0 L of H₂ (g)(MW = 2.016) are produced at 20 ⁰C,Calculate the pressure of H₂ gas.

Question 2. Calculate the heat released when 84.5g of SO₂  (MW = 64.07) are used up according to the following equation.  2 SO_2(g) + O₂(g) + O(g)   →   2SO_2(g)  Δ_H^o = 99.1kJ

Question 3. Calculate the  Δ_T   for a 87.5 g piece of copper when one adds 2.1kJ of heat energy to that piece of cooper. Copper has a specific heat capacity of 0.385 J/g ⁰C.

Question 4. Write the thermo chemical equation for the standard enthalpy of formation of solid ammonium chloride,NH₄Cl,given that the reaction releases 314 kilojoules per mole of ammonium chloride.

Question 5. In an instant cold pack(used to treat athletic injuries),50.0g of NH₄NO₃ is mixed with 125 g of H₂O at an initial temperature of 25.00^°C.After the dissolving of the salt, the final temperature of the solution is 3.10 ⁰C.

Calculate the enthalpy change for the dissolution of NH₄NO₃ in Kj/mol.Assume that the masses are addictive .Also ,assume that the heat capacity of the calorimeter is zero and the solution has specific heat of 4.18J/g ⁰C.

NH₄NO₃ (s) →    H₂O   →   NH₄NO₃ (aq)

Question 6. Calculate the Δ_H^°  for this reaction 3 NO_{2 (g) +}  H₂0 (l)   →    2HNO₃ (aq) + NO (g).

Question 7. Typical atmospheric pressure on Mt.Everest (29,028 ft) is 235 mm Hg.Convert this pressure to atm and in Hg.

Question 8. A 3.50 L flask contains 7.65 g methane (CH₄   MW = 16.04) at 27 ⁰C.Calculate the pressure (in atm) inside the flask.

Question 9. A gas sample is heated from -10⁰C to 57.0 ⁰C and the volume is increased from 2.00 L to 4.5 L .If the initial pressure is 0.425 atm, calculate the new pressure of the gas.

Question 10. A gas consist of only carbon and hydrogen has an empirical formula of CH_3. The gas has a density of 3.32 g/L at 27.0 ⁰ C and 739 mm Hg.

a) Calculate the molar mass of the gass

b) Determine the molecular formula of the gas

Question 11. Calculate the Δ_H  for this reaction:

 2 C(s) + H_{2 (g)   →}   C₂H₂(g)

Given the following data

C₂H₂(g) + ^5/2 O_{2(g)    →}   2CO_{2 (g) +}  H₂O(l)    Δ_{H  = -1299.6} kJ

C (s) + O_{2 (g)   →}  CO₂(g)                                 Δ _{H =  - 393.5 kJ}

H_{2(g)  +} ^1/2O_{2(g)    →}   H₂O(l)                           Δ _{H   =}  -285.9 kJ

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