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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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If the initial mixture of reactants for CO(g) + 2H2(g) → CH3OH(g) contains 4.00 moles of CO and 4.00 moles of H2, what is the limiting reactant and how many moles of methanol can be produced?
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- if 5.7kg of CO2 are produced during a combustion reaction, how many molecules of Co2 would be produced?arrow_forwardNitrogen and hydrogen react to form ammonia according to the following balanced equation: N2(g) + 3H2(g) → 2NH3(g) Calculate the number of moles of hydrogen required to react with 0.0883 mole of nitrogen, and the number of moles of ammonia that will form. Determine the mass of CO2 and the mass of H2O produced by the combustion of 1.55 g of a compound with the empirical formula CH4O. What is the mass of CO2? What is the mass of H2O?arrow_forwardAspirin (C9H8O4) is synthesized by reacting salicyclic acid (C7H6O3) with acetic anhydride (C4H6O3). The chemical equation is: C7H6O3 + C4H6O3 ⟶ C9H8O4 + HC2H3O2 If we react 100. g of acetic anhydride with 100. g of salicyclic acid, what mass of aspirin do we expect to produce if the percent yield for this reaction coms out to 84%?arrow_forward
- The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: 2 NO(g) + O2(g) – 2 NO2(g) If 9.500 g NO is mixed with 11.99 g 02, calculate the theoretical yield (g) of NO2 produced by the reaction.arrow_forwardDetermine the limiting reactant (LR) and the Theoretical Yield (in g) of nitrogen that can be formed from 58.0 g N2O4 and 40.0 g N2H4. Some possibly useful molar masses are as follows: N2O4= 92.02 g/mol, N2H4= 32.05g/mol. N2O4(l) + 2 N2H4 --------> (l) 3 N2(g) + 4 H2O(g)arrow_forward3N2 (g) + H2(g) ~> 2NH3(g) is the balanced chemical equation for the synthesis of ammonia. If an manufacturer uses 6 moles of nitrogen gas as a starting amount, how many moles of ammonia will they produce?arrow_forward
- Consider the following balanced equation: 6HCl(aq) + 2Al(s) → 3H2(g) + 2AlCl3(s) If 1.72×102 moles of HCl(aq) and 48.8 moles of Al(s) are allowed to react to produce 60.2 moles of H2(g), what is the percent yield of the reaction?Provide your answer in decimal notation, rounded to 1 decimal digit.arrow_forwardUse the equation, 2C4H10 + 13O2 arrow 8CO2 + 10H2), to determine the moles of oxygen required to react 3.4 moles of butane( C4H10).arrow_forwardIf 6.5 kg of CO₂ are produced during a combustion reaction, how many molecules of CO₂ would be produced?arrow_forward
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