Which of the following is a nonrenewable resource?

A. Petroleum

B. Biomass

C. Hydropower

D. Solar

Consider the following equilibrium: O2 (g) + 2F2 (g) ↔ 2OF2 (g); Kp = 2.3*10-15 Which of the following statements is true? a.

Consider the reaction: 2 SO2 (g) + O2 (g) 2 SO3. If, at equilibrium at a certain temperature, [SO2] = 1.50 M, [O2] = 0.120 M, and [SO3] = 1.25 M, what is the value of the equilibrium constant? none of the above 8.68 6.94 0.14 5.79

A 49.48-mL sample of an ammonia solution is analyzed by titration with HCl. It took 38.73 mL of 0.0952 M HCl to titrate the ammonia. What is the concentration of the original ammonia solution?

At constant pressure, which of these systems do work on the surroundings? A (s) + B (s) ⟶ C (g) A (s) + B (s) ⟶C (g) 2 A (g) + 2 B (g) ⟶ 5 C (g) 2A (g) + 2B (g) ⟶5C (g) A (g) + B (g) ⟶ C (g) A (g) + B (g) ⟶C (g) 2 A (g) + 2 B (g) ⟶ 3 C (g)

Weird type of bond. (show work) Agl CdSn HS Pb2S2 Cl2 KSn TIO2

Glucose is not made from which of the following

Rank the temperatures from the highest to the lowest. 133F 351K 25C 273K 146C 58F 95F

Calculate the density of sulfuric acid if 35.4 mL of the acid weighs 65.14 g.

Where the single machos?

A reaction will be spontaneous only at low temperatures if both ΔH and ΔS are negative. For a reaction in which ΔH = - 320.1 kJ/mol and ΔS = - 86.00 J/K · mol. Determine the temperature (in °C) below which the reaction is spontaneous.