Consider the Haber process shown below. N2 (g) + 3 H2 (g) → 2 NH3 (g) Which of the following statements IS NOT TRUE? Assume 100% yield. a. 15 moles of nitrogen gas react with 45 moles of hydrogen gas to form 30 moles of ammonia gas. b. 5 molecules of nitrogen gas react with 15 molecules of hydrogen gas to form 10 molecules of ammonia gas. c. 25 grams of nitrogen gas react with 75 grams of hydrogen gas to form 50 grams of ammonia gas. d. 28 grams of nitrogen gas react with 6 grams of hydrogen gas to form 34 grams of ammonia gas.

5. Complete and balance the following combustion reactions. (You will need to determine the molecular formulas of the reactants.) а. pentane + О2 b. toluene + O2 c. cyclohexene + O2

5. Provide a balanced chemical equation, be sure to include state designations. a. Hydrogen and oxygen react to form steam. b. In an aqueous solution, zinc acetate and sodium sulfide are mixed. c. Lithium and bromine react. d. Combustion of liquid butane (C4H10). e. Dilute sulfuric acid is added to a solution of aluminum hydroxide. f. Decomposition of potassium chlorate.

1. A reaction at 21.7 ˚C and 1.03 atm produces 18.0 L of CO2 (g). Determine the number of moles of CO2 (g) produced. 2. Determine the volume (mL) of C2H5OH (l) that was combusted to produce the volume of CO2 (g) collected above. The density of C2H5OH (l) is 0.789 g/mL

. For each reaction scenario below, predict the products of the reaction, and write a complete balanced chemical equation. If you predict that no reaction will occur, write the reactants, then write NR after the arrow. а. Water undergoes decomposition by electrolysis. b. A table salt (sodium chloride) solution is poured into an aluminum can. с. A copper (II) nitrate solution is combined with an ammonium chromate solution.

1. Consider the generic reaction: A + 2B→ CHow many moles of C are formed upon the complete reaction of:A. 5.0 moles of AB. 5.0 moles of B 2. For the reaction: 2N2O5 → 4NO2 + O2Calculate how many moles of NO2 form when each amount of the reactant completely reacts.A. 1.3 moles N2O5B. 1.006x10-3 mole N2O5 3. For the reaction: 2S + 3O2 → 2SO3A. Calculate the moles of S needed to completely react with 1.75 moles of O2B. Calculate the moles of product that form when 1.75 moles of O2 completely reacts. Assume thereis more than enough S. 4. For the reaction: 2S + 3O2 → 2SO3A. Calculate the mass of S (32.07 g/mol) needed to completely react with 5.3 g of O2 (32.00 g/mol).B. Calculate the mass of SO3 (80.07 g/mol) that form when 5.3 g of O2 completely reacts. Assumethere is more than enough S. 5. A mixture containing 21 moles of F2 and 8 moles of S is allowed to react according to the reaction:3F2 + S → SF6A. What is the limiting reactant?B. How many moles of the excess reactant remain after…

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diagram b is correct,     What procedures can be used to solve this problem? write down the plan for this new way to solve the problem.  1. first execute plan 1 to solve this problem. explain in every step. 2. solve the problem again - this time use the plan that you propose, plan 2. 3. finally, think about the way that you can use it to make sure that your answer makes sense. write your assessment.

In experiment #7, you observed the formation of carbon dioxide by reacting baking soda with vinegar.  Why was it not possible to relight the candle? A. Carbon dioxide is heavier than air so it stays in the beaker preventing the candle from relighting. B. Carbon dioxide is lighter than air so it escaped from the beaker and the candle should have relit. C. Carbon dioxide is heavier than air so it stays in the beaker and the candle should have relit. D. Carbon dioxide is lighter than air so it escaped from the beaker preventing the candle from relighting.

Consider the synthesis of ammonia: N2 (g) +3H, (g) 2NH3 (g)