Carbon disulfide is a foul-smelling solvent that dissolves sulfur and other nonpolar substances. It can be...
Carbon disulfide is a foul-smelling solvent that dissolves sulfur and other nonpolar substances. It can be made by heating sulfur in an atmosphere of methane. For the reaction (below), ΔHrxn° = 760.4 kJ and ΔSrxn°= 1219.1 J/K.
4CH4 (g) + S8 (s) <----> 4CS2 (g) + 8H2 (g)
Calculate the equilibrium constant at 250.0 °C.
AND...
Calculate the equilibrium constant at 500.0°C.
Homework Answers
k = 4.97 ×
10-13
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Carbon disulfide is a foul-smelling solvent that dissolves
sulfur and other nonpolar substances. It can be...
Carbon disulfide is a foul-smelling solvent that dissolves sulfur and other nonpolar substances. It can be...
Carbon disulfide is a foul-smelling solvent that dissolves sulfur and other nonpolar substances. It can be made by heating sulfur in an atmosphere of methane. For the reaction (below), AHrxn° = 760.4 kJ and ASrxnº= 1219.1 J/K. 4CH_(8) +Sg(s) – 4CS2(g) +8H2(g) 1st attempt Part 1 (1 point) . See Periodic Table Calculate the equilibrium constant at 250.0 °C. Part 2 (1 point) See Hint Calculate the equilibrium constant at 500.0°C.
Resources Give Hint Check Ans n2 of 5 > Carbon disulfide is prepared by heating sulfur...
Resources Give Hint Check Ans n2 of 5 > Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S (8) + C(s) - CS (8) Ke = 9.40 at 900 K How many grams of CS (8) can be prepared by heating 9.30 mols, (g) with excess carbon in a 6.15 L reaction vessel held at 900 K until equilibrium is attained? 1 mass of CS, (g): General Chemistry | Publisher: Un about us Careers Privacy...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2 (g)+ C(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2 (g)+ C(s) -->CS2 (g) Kc = 9.40 at 900K How many grams of CS2(g) can be prepared by heating 15.5 moles of S2(g) with excess carbon in a 8.15 L reaction vessel held at 900 K until equilibrium is attained?
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is s_2(g) + c(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is s_2(g) + c(s) CS_2(g) k_c = 9.40 at 900 K How many grams of CS_2(g) can be prepared by heating 21.1 moles of S_2(g) with excess carbon in a 9.35 L reaction vessel held at 900 K until equilibrium is attained?
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS (8) K. = 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 17.9 mol S2(g) with excess carbon in a 7.90 L reaction vessel held at 900 K until equilibrium is attained?
THALPY, ENTROPY, AND FREE ENERGY Carbon disulfide, CS2, is a toxic, highly flammable substance that is an excellent solvent for large, nonpolar, organic species such as fats, resins, rubber...
THALPY, ENTROPY, AND FREE ENERGY Carbon disulfide, CS2, is a toxic, highly flammable substance that is an excellent solvent for large, nonpolar, organic species such as fats, resins, rubbers, and asphalt. The following thermodynamic data are available for CS, (g) and CS, (1) at 298 K: CS2 (8) CS2 (D) 67.2 65.3 89.7 a) Liquid CS, burns in oxygen with a blue flame, forming CO,(8) and SO, (g). Write a balanced chemical equation for this reac tion. Calculate the ΔΗΡ...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS (8) K = 9.40 at 900 K How many grams of CS, (g) can be prepared by heating 17.8 mol S. (g) with excess carbon in a 7.30 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(g):
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS, (g) Kc = 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 11.4 mol S2(g) with excess carbon in a 5.15 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g): bun
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g) + C(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g) + C(s) = CS, (g) Kc = 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 11.8 mol S2(g) with excess carbon in a 6.15 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g): 09
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS, (g) Kc = 9.40 at 900 K How many grams of CS, (g) can be prepared by heating 15.5 mol S, (g) with excess carbon in a 7.40 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g): g At a certain temperature, the Kp for the decomposition of H. S is 0.752. HS(g) =H2(g) + S(g) Initially,...
Carbon disulfide is a foul-smelling solvent that dissolves sulfur and other nonpolar substances. It can be made by heating sulfur in an atmosphere of methane. For the reaction (below), AHrxn° = 760.4 kJ and ASrxnº= 1219.1 J/K. 4CH_(8) +Sg(s) – 4CS2(g) +8H2(g) 1st attempt Part 1 (1 point) . See Periodic Table Calculate the equilibrium constant at 250.0 °C. Part 2 (1 point) See Hint Calculate the equilibrium constant at 500.0°C.
Resources Give Hint Check Ans n2 of 5 > Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S (8) + C(s) - CS (8) Ke = 9.40 at 900 K How many grams of CS (8) can be prepared by heating 9.30 mols, (g) with excess carbon in a 6.15 L reaction vessel held at 900 K until equilibrium is attained? 1 mass of CS, (g): General Chemistry | Publisher: Un about us Careers Privacy...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is s_2(g) + c(s) CS_2(g) k_c = 9.40 at 900 K How many grams of CS_2(g) can be prepared by heating 21.1 moles of S_2(g) with excess carbon in a 9.35 L reaction vessel held at 900 K until equilibrium is attained?
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS (8) K. = 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 17.9 mol S2(g) with excess carbon in a 7.90 L reaction vessel held at 900 K until equilibrium is attained?
THALPY, ENTROPY, AND FREE ENERGY Carbon disulfide, CS2, is a toxic, highly flammable substance that is an excellent solvent for large, nonpolar, organic species such as fats, resins, rubbers, and asphalt. The following thermodynamic data are available for CS, (g) and CS, (1) at 298 K: CS2 (8) CS2 (D) 67.2 65.3 89.7 a) Liquid CS, burns in oxygen with a blue flame, forming CO,(8) and SO, (g). Write a balanced chemical equation for this reac tion. Calculate the ΔΗΡ...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS (8) K = 9.40 at 900 K How many grams of CS, (g) can be prepared by heating 17.8 mol S. (g) with excess carbon in a 7.30 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(g):
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS, (g) Kc = 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 11.4 mol S2(g) with excess carbon in a 5.15 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g): bun
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g) + C(s) = CS, (g) Kc = 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 11.8 mol S2(g) with excess carbon in a 6.15 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g): 09
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) = CS, (g) Kc = 9.40 at 900 K How many grams of CS, (g) can be prepared by heating 15.5 mol S, (g) with excess carbon in a 7.40 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g): g At a certain temperature, the Kp for the decomposition of H. S is 0.752. HS(g) =H2(g) + S(g) Initially,...
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