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parts a & b
(34.) The decomposition reaction of carbon disulfide, CS, to carbon monosulfide, CS,...
The decomposition reaction of carbon disulfide, CS, to carbon monosulfide, CS, and sulfur is first order with k = 2.8 x 10-75-1 at 1000°C. CS, - → CS + S (a) What is the half-life of this reaction at 1000°C? (b) How many days would pass before a 2.00-gram
The decomposition reaction of carbon disulfide, CS, to carbon monosulfide, CS, and sulfur is first order with k = 2.8 x 10-75-1 at 1000°C. CS, - → CS + S (a) What is the half-life of this reaction at 1000°C? (b) How many days would pass before a 2.00-gram sample of CS, had decomposed to the extent that 0.75 gram of T. CS, remained? (c) Refer to part (b). How many grams of CS would be present after this length...
chemistry
The decomposition reaction of carbon disulfide, CS, to carbon monosulfide, CS, and sulfur is first order with k = 2.8 x 10-75-1 at 1000°C. CS, - → CS + S (a) What is the half-life of this reaction at 1000°C? (b) How many days would pass before a 2.00-gram sample of CS, had decomposed to the extent that 0.75 gram of T. CS, remained? (c) Refer to part (b). How many grams of CS would be present after this length...
Carbon disulfide is produced by the reaction of carbon and sulfur dioxide. 5C(s) + 280,(9)-CS (9)...
Carbon disulfide is produced by the reaction of carbon and sulfur dioxide. 5C(s) + 280,(9)-CS (9) + 4CO(9) Part A What is the percent yield of carbon disulfide if the reaction of 40.3 g of carbon produces 34.0 g of carbon disulfide? Express your answer with the appropriate units. The percent yield of CS2 = Value Units Submit Request Answer Part B What is the percent yield of carbon disulfide if the reaction of 33.8 g of sulfur dioxide produces...
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 S() + C(s)...
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S() + C(s) - 0S,(8) Ke-9.40 at 900 K How many grams of CS,(s) can be prepared by heating 19.0 mol S, () with excess carbon in a 9.00 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(8):
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 How many grams...
Carbon disulfide is prepared by heating sulfur and charcoal. The
chemical equation is
How many grams of CS2(g) can be prepared by heating 10.8 moles
of S2(g) with excess carbon in a 5.30 L reaction vessel held at 900
K until equilibrium is attained?
rbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is 9.40 at 900 K CS How many grams of g) can be prepared by heating 10.8 moles of S2(g) with excess carbon in...
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 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?
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 produced by the reaction of carbon and sulfur dioxide. 5C(s) + 280,(9)-CS (9) + 4CO(9) Part A What is the percent yield of carbon disulfide if the reaction of 40.3 g of carbon produces 34.0 g of carbon disulfide? Express your answer with the appropriate units. The percent yield of CS2 = Value Units Submit Request Answer Part B What is the percent yield of carbon disulfide if the reaction of 33.8 g of sulfur dioxide produces...
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() + C(s) - 0S,(8) Ke-9.40 at 900 K How many grams of CS,(s) can be prepared by heating 19.0 mol S, () with excess carbon in a 9.00 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(8):
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
How many grams of CS2(g) can be prepared by heating 10.8 moles
of S2(g) with excess carbon in a 5.30 L reaction vessel held at 900
K until equilibrium is attained?
rbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is 9.40 at 900 K CS How many grams of g) can be prepared by heating 10.8 moles of S2(g) with excess carbon in...
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 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?
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
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