A. Starting with 500 g of N2 and 500 g of H2 how much NH3 can...

A. Starting with 500 g of N2 and 500 g of H2 how much NH3 can you form? And how much of the excess reagent ( N2 or H2) remains (eg. is left over) after the reaction goes to completion?

B. Starting with 50 g of sulfuric acid and 40 g of baking soda, how much sodium sulfate is produced?

C. Based on the information in 6d above, how much of the excess reactant remains after the reaction has gone to completion?

Expert Solution

queen_honey_blossom answered 8 months ago

3H2(g)+N2(g)?2NH3(g) How many grams of NH3 can be produced from 3.23mol of N2 and excess H2....

3H2(g)+N2(g)?2NH3(g) How many grams of NH3 can be produced from 3.23mol of N2 and excess H2. How many grams of H2 are needed to produce 13.85g of NH3? How many molecules (not moles) of NH3 are produced from 6.68

Consider the reaction: 3 H2 (g) + N2 (g) ⇋ 2 NH3 (g) In a given...

Consider the reaction: 3 H2 (g) + N2 (g) ⇋ 2 NH3 (g) In a given reaction, the initial concentrations of reactants and product are: [H2] = 0.150 M; [N2] = 0.300 M ; [NH3] = 0.000 M If the equilibrium concentration of H2 is 0.0900 M, what is Kc for the reaction under these conditions?

Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts...

Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts with 18 g of H2(g). d. What is the limiting reactant? e. When the reaction is complete, how many grams of NH3(g) are produced? f. When the reaction is complete, how many grams of N2(g) remain? g. When the reaction is complete, how many grams of H2(g) remain? h. If the reaction actually produced 55 g of NH3(g), what is the percent yield?

1.38 g H2 is allowed to react with 10.2 g N2 , producing 2.64 g NH3...

1.38 g H2 is allowed to react with 10.2 g N2 , producing 2.64 g NH3 .

At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches...

At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10^−2 atm, respectively. (a) Compute the value of the equilibrium constant, KP at 400K. (b) Compute the standard Gibbs free energy of this reaction at 400K. Express the result in kJ/mol. (c) Would the system be at equilibrium at 400 K if the partial pressures...

1.28 g H2 is allowed to react with 9.54 g N2, producing 1.31 g NH3. Part...

1.28 g H2 is allowed to react with 9.54 g N2, producing 1.31 g NH3. Part A: What is the theoretical yield in grams for this reaction under the given conditions? Part B: What is the percent yield for this reaction under the given conditions?

1.30 g H2 is allowed to react with 10.4 g N2, producing 2.53 g NH3. What...

1.30 g H2 is allowed to react with 10.4 g N2, producing 2.53 g NH3. What is the theoretical yield in grams for this reaction under the given conditions? What is the percent yield for this reaction under the given conditions?

1.44 g H2 is allowed to react with 9.95 g N2, producing 1.79 g NH3. What...

1.44 g H2 is allowed to react with 9.95 g N2, producing 1.79 g NH3. What is the theoretical yield for this reaction under the given conditions?

1.44 g H2 is allowed to react with 9.56 g N2, producing 2.46 g NH3. What...

1.44 g H2 is allowed to react with 9.56 g N2, producing 2.46 g NH3. What is the theoretical yield? What is the percent yield?

Consider the reaction 2 NH3 (g) ? N2 (g) + 3 H2 (g). Suppose 6 moles...

Consider the reaction 2 NH3 (g) ? N2 (g) + 3 H2 (g). Suppose 6 moles of pure ammonia are placed in a 1.0 liter flask and allowed to reach equilibrium. If X represents the concentration (in M) of nitrogen present in the system once equilibrium is reached, which of the following will represent the concentration of ammonia in M? Show work A) 6

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