Use the References to access important values if needed for this question. The following information is given for lead at 1 atm: boiling point = 1740 °C melting point = 328 °C AHvap(1740 °C) = 177.8 kJ/mol AHfus (328 °C) = 4.77 kJ/mol specific heat solid = 0.130 J/g°C specific heat liquid = 0.138 J/g°C What is AH in kJ for the process of freezing a 39.5 g sample of liquid lead at its normal melting point of 328 °C? kj

The lattice energy is defined as the energy required to break one mole of an ionic solid into its ions in the gas phase. The lattice energy for calcium oxide corresponds to the following reaction. CaO(s) Ca2+(g) + O2-(g) DH = ? Using the following information, determine the lattice energy for calcium oxide. Ca(s) ----> Ca(g) DH = 178.2 kJ Ca(g) ----> Ca2+(g) + 2e-   DH = 1747.9 kJ O2(g) ----> 2O(g) DH = 498.3 kJ O2-(g) ----> O(g) + 2e- DH = -702 kJ Ca(s) + 1⁄2 O2(g) ----> CaO(s)   DH = -635.0 kJ   Using the unrounded answer from the previous problem determine q (kJ) for the following reaction when 1.00 grams of solid calcium oxide forms.     Ca2+(g) + O2-(g) ⟶⟶ CaO(s)

The temperature of a sample of iron increased by 22.0 °C22.0 °C when 269 J269 J of heat was applied. What is the mass of the sample?   Substance Specific heat J/(g · °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903

IT The temperature of a sample of aluminum increased by 24.6 °C when 255 J of heat was applied. Substance Specific heat J/(g lead 0.128 What is the mass of the sample? silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 m =

The following information is given for bismuth at 1 atm: Tb 1627.00°C AHvap (1627.00°C) = 822.9 J/g = Tm = 271.00°C AHfus (271.00°C) = 52.60 3/g Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C A 46.90 g sample of solid bismuth is initially at 253.00°C. If 3.332 x 10³ J of heat are added to the sample at constant pressure ( P = 1 atm), which of the following is/are true? (Select all that apply.) The sample is a gas. The sample is at a temperature of 271.00°C. The sample is at a temperature greater than 271.00°C. The sample is a liquid. The sample is a solid in equilibrium with liquid.

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)

How many grams of an unknown substance, having a specific heat of 1.66 J g ° C, are present if a temperature change of -173.4 K occurs. The heat lost was 35981 J.

Using the following thermochemical data: 2Er(s) + 6HF(g) → 2ErF3(s) + 3H2(g) ΔH° = -1795.4 kJ/mol 2Er(s) + 6HCl(g) → 2ErCl3(s) + 3H2(g) ΔH° = -1443.6 kJ/mol calculate ΔH° for the following reaction:ErF3(s) + 3HCl(g) → ErCl3(s) + 3HF(g) 351.8 kJ/mol -3239.0 kJ/mol -1619.5 kJ/mol 703.6 kJ/mol 175.9 kJ/mol

Given the following thermochemical equation, what is the standard heat of formation for NaOH? 2NaOH(s)-->2Na (s) + O2 (g) + H2 (g) TriangeH= +875.6 kJ a) 875.6 kJ b) -875.6 kJ c) 437.6 kJ d) -437.6 kJ e) 1751.1 kJ f) -1751.1 kJ

Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. How much heat, in J, was absorbed by the water assuming the specific heat of the water is 4.184 J/g･°C?