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The equilibrium constant of the chemical reaction at 373 K is 0.75. If the initial concentration of N2O4 (reactant) is 0.50 M, what is the equilibrium concentration of NO2 (product)?
Solve the equilibrium constant of the given chemical equation, CO2(g) ⇌ CO(g) + O2(g), if the molar concentrations are CO2 = 1.75 M, CO = 1.00 M, and O2 = 0.25 M.
Given the following data, calculate ∆G for this chemical reaction, CH4 + 2O2 → CO2 + 2H2O, if H = 750 J , S = 25.75 J/K, and T = 315 K.
Calculate the entropy of chemical reaction that takes place between a hydrogen and chlorine gas if H = 125 J , G = 500 J, and T = 250 K.
Solve the equilibrium concentration of Cl2 from the given chemical equation: PCl3(g) + Cl2(g) ⇌ PCl5(g). (PCl3 = 0.50 M; PCl5 = 1.25 M; K = 0.75 M)
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Solve the equilibrium constant of the given chemical equation, 2S(s) + 3O2(g) ⇌ 2SO3(g), if the molar concentration of oxygen gas is 1.25 M and of sulfite is 1.75 M.
If the temperature remains constant in C2H2 + O2 ⇆ CO2 + H20 ΔH = +
If the pressure increases by half in C2H2 + O2 ⇆ CO2 + H20 ΔH = +
If the amount of CO2 increases in C2H2 + O2 ⇆ CO2 + H2O ΔH = +
What is the mass in milligrams of 7.40× 10 to the power of 20 molecules of dinitrogen trioxide
