Given the following equations, find the AHºf of one mol of HCI from its elements. Show the balanced chemical equation for the formation of HCl from H2 and Cl2. Target Equation: A) N2 (g) + 3 H2 (g) → 2 NH3 (g) AH°rxn = -91.8 kJ B) N2 (g) + 4 H2 (g) + Cl2 (g) → 2 NHẠCI (s) AH°, rxn = -628.8 kJ C) NH3 (g) + HCI (g) → NHẠCI (s) AH°rxn = -176.2 kJ

Calcium carbonate can be decomposed upon applying heat with the following equation CaCO3(s)  →  CaO(s)  +  CO2(g)    ΔH = +179.5kJ How much heat will be needed to decompose 30 g of calcium carbonate?  AND What size container will be required (in L) to contain the carbon dioxide generated at 25ºC and 1.2 atm?

4. Consider the equations for these reactions: % N2 + % O2 → NO NO2 → NO + % 02 AH = +90.4 kJ AH = +56.5 All reactants are gaseous. What is the heat of formation (AH;) for NO2 gas?

Use the following information to calculate the amount of heat involved in the complete reaction of 7.20 g of carbon to form PbCO3(s) in reaction 4. Be sure to give the proper sign (positive or negative) with your answer. Reaction 1 Pb(s) + O₂(g) PbO(s) Reaction 2 C(s,graphite) + O₂(g) →→→ CO₂(g) Reaction 3 PbCO3(s). PbO(s) + CO₂(g) Reaction 4 Pb(s) + C(s,graphite) + O₂(g) →→→ PbCO3(s) 1st attempt AH rxn4° = ? kJ AH rxnl AHO rxn2 AHO rxn3 AHXn4 = -219 kJ = - 394 kJ = 86 kJ = ? See Periodic Table See Hint

Octane (C8H18) is a component of gasoline that burns according to the following equation:  C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?

Which chemical reaction below yields the heat of formation of liquid ammonia (NH3)? 3H(g) + N(g) →→→ NH3(e) H₂ (g) + N2₂ (g)→→ NH3(e) 3/2 H₂ (g) + 1/2 N₂ (g)→ NH3 (e) 3H₂(g) + N₂ (g)→ 2NH3(e) 3/2 H₂(g) + N(g)→ NH3(e)

Calculate the heat required  to raise the temperature of a 50.0 g of water from 25.0 °C to 39.0 °C. (The specific heat capacity of water is 4.184 J·g–1·°C–1). A) 2.93 kJ B) 4.18 kJ C) 5.23 kJ D) 8.16 kJ         0.163 kJ

Suppose 2.32 kJ of heat is added to 25.4 g of ethanol at 18.71 °C. The specific heat capacity of ethanolis 2.46 J/g °C. What is the final temperature of the ethanol?

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

The overall reaction in commercial heat packs can be represented as 4Fe(s) + 302(g) →2Fe₂O3 (8) AH = -1652 kJ a. How much heat is released when 2.20 mol iron is reacted with excess O₂? kl released b. How much heat is released when 1.83 mol Fe2O3 is produced? kJ released c. How much heat is released when 2.20 g iron is reacted with excess O₂? kJ released d. How much heat is released when 11.8 g Fe and 2.61 g O2 are reacted? Submit Answer [Review Topics] kl released Retry Entire Group [References] 8 more group attempts remaining