An unknown liquid is 1.003x104 Pa at 25°C and 7.438x104 Pa at 50 °C. has the x kJ/mol enthalpy of vaporization (ΔHvap), based on the Clausius-Clapeyron equation. What is the value of x in 3 significant figures?

Substance X is known to exist at 1atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined (picture). You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at -20°C is put into an evacuated flask and heated at a constant rate until 10 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment.

Calculate the amount of heat needed to boil 87.1 g of acetic acid (HCH3CO2), beginning from a temperature of 56.6 C. Be sure your unit has a unit symbol and the correct number of significant digits.

How many grams of C6H6 must decompose according to the following chemical equation to transfer 430KJ of heat? C₆H₆(l) → 3C₂H₂(g) ∆H = 630KJ

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 amount of heat (in kJ) is required to convert 10.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g. °C; specific heat capacity of gas = 0.932 J/g⋅ °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3 °C)

Calculate the heat required to bring 10.0 g CCl2F2 from -29.8°C as a liquid to the gas phase at 10.0°C. (molar mass = 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K ΔHvap = 20.1 kJ/mol ΔHfus = 4.14 kJ/mol

How many grams of C₆H₆ must decompose according to the following chemical equation to transfer 430 kJ of heat? C₆H₆(l) → 3 C₂H₂(g) ∆H = 630 kJ

A 0.580 g0.580 g sample of steam at 107.3 ∘C107.3⁢ ∘C is condensed into a container with 4.56 g4.56 g of water at 17.0 ∘C.17.0⁢ ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18  J g⋅ ∘C,4.18  J g⋅ ∘C, the specific heat of steam is 2.01  J g⋅ ∘C,2.01  J g⋅ ∘C, and Δ?vap=40.7 kJ/mol.