Which one of the following statements is NOT true concerning the equation below? N2(g) + 3...
Which one of the following statements is NOT true concerning the
equation below?
N2(g) + 3 H2(g) → 2 NH3(g) ΔH°rxn = -459.0 kJ
A) The production of 1.00 mole of ammonia is accompanied by the
production of 229.5 kJ of heat.
B) The complete reaction of 1.00 moles of nitrogen requires 459 kJ
of heat.
C) The complete reaction of 1.00 moles of hydrogen produces 153 kJ
of heat.
D) The complete reaction of 0.8278 moles of hydrogen requires
0.2759 moles of nitrogen.
E) The reaction is exothermic
Homework Answers
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Which one of the following statements is NOT true concerning the
equation below?
N2(g) + 3...
The following ia a balanced reaction N2 (g) + 3 H2 (g)2 N We read the...
The following ia a balanced reaction N2 (g) + 3 H2 (g)2 N We read the above reaction as follows: 1 mole of N2 (nitrogen)reacts with 3 moles of H2 (hydrogen) to form 2 moles of NH3 (ammonia). Which statement is correct (a) 14.0 g of nitrogen reacts with reacts with 6.0 g of hydrogen to form 34.0 g ammonia (b) 28.0 g of nitrogen reacts with 6.0 g hydrogen to form 17.0 g ammonia (c) 14.0 g of nitrogen...
Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g)...
Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g) → 2 NH3(g). The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AG at 50.00°C for the preparation of 2 moles of NH3. (answer in kJ/mol) Answer: -56.723 Check
Mole Relationships in Chemical EquationsAmmonia is produced by the reaction of hydrogen and nitrogen.N2(g) + 3H2(g)...
Mole Relationships in Chemical EquationsAmmonia is produced by the reaction of hydrogen and nitrogen.N2(g) + 3H2(g) → 2NH3(g) ammoniaa. How many moles of H2 are needed to react with 1.0 mole N2?b. How many moles of N2 reacted if 0.60 mole NH3 is produced?c. How many moles of NH3 are produced when 1.4 moles H2 reacts?
26.) Ammonia is produced by the reaction of hydrogen and nitrogen as follows: N2(g)+3H2(g)→2NH3(g)ammonia Express the...
26.) Ammonia is produced by the reaction of hydrogen and nitrogen as follows: N2(g)+3H2(g)→2NH3(g)ammonia Express the number of moles to two significant figures. (A.) How many moles of H2 are needed to react with 1.0 mol of N2? (B.) How many moles of N2 reacted if 0.50 mol of NH3 is produced? (C.) How many moles of NH3 are produced when 1.7 mol of H2 reacts?
6. Use the following thermochemical equation for the synthesis of ammonia N2(g) + 3 H2(g) →...
6. Use the following thermochemical equation for the synthesis of ammonia N2(g) + 3 H2(g) → 2 NH3(g) AH = -91.8 kJ Rewrite the thermochemical equation to show 3 moles of hydrogen being produced? Rewrite the thermochemical equation to show 6 moles of hydrogen being produced? Rewrite the thermochemical equation to show the production of 6 moles of NH3 produced? 7. Use the thermochemical equation below to find the AH of the following: CH_(g) + H2O(g) → CO(g) + 3...
Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How...
Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How many moles of NH3 can be produced from 18.0 mol of H2 and excess N2? Express the number of moles to three significant figures
The production of ammonia from nitrogen and hydrogen: N2(g) 3 H2gNH3(g) is an exothermic reaction: when...
The production of ammonia from nitrogen and hydrogen: N2(g) 3 H2gNH3(g) is an exothermic reaction: when 10.0 g of ammonia are produced in a bomb calorimeter, the temperature rises 3.92°C Determine the internal energy change (kJ mol-1) of this reaction. Take Ceal 3.07 kJ/oC h.s TARIS WTH THD.OR
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. Given that the standard enthalpy of the reaction at 400K is DH = -94 kJ/mol, estimate the value of the equilibrium constant KP at 450 K assuming that the standard enthalpy of reaction does not vary significantly with temperature in this temperature...
The Haber-Bosch process is used to make ammonia from nitrogen and hydrogen: N2(g) + 3 H2(g)...
The Haber-Bosch process is used to make ammonia from nitrogen and hydrogen: N2(g) + 3 H2(g) 2 NH3(g). A 10.0 L reactor at 450 °C is filled with 3 moles of nitrogen and 12 moles of hydrogen, K is 0.16 under these conditions.
N2 (g) + 3 H2 (g) -> 2 NH3 (g) assume 0.210 mol N2 and 0.674...
N2 (g) + 3 H2 (g) -> 2 NH3 (g) assume 0.210 mol N2 and 0.674 mol H2 arw present initially. after complete reaction, how many moles of ammonia are produced? how many moles of H2 remain? how many moles of N2 remain?
The following ia a balanced reaction N2 (g) + 3 H2 (g)2 N We read the above reaction as follows: 1 mole of N2 (nitrogen)reacts with 3 moles of H2 (hydrogen) to form 2 moles of NH3 (ammonia). Which statement is correct (a) 14.0 g of nitrogen reacts with reacts with 6.0 g of hydrogen to form 34.0 g ammonia (b) 28.0 g of nitrogen reacts with 6.0 g hydrogen to form 17.0 g ammonia (c) 14.0 g of nitrogen...
Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g) → 2 NH3(g). The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AG at 50.00°C for the preparation of 2 moles of NH3. (answer in kJ/mol) Answer: -56.723 Check
6. Use the following thermochemical equation for the synthesis of ammonia N2(g) + 3 H2(g) → 2 NH3(g) AH = -91.8 kJ Rewrite the thermochemical equation to show 3 moles of hydrogen being produced? Rewrite the thermochemical equation to show 6 moles of hydrogen being produced? Rewrite the thermochemical equation to show the production of 6 moles of NH3 produced? 7. Use the thermochemical equation below to find the AH of the following: CH_(g) + H2O(g) → CO(g) + 3...
The production of ammonia from nitrogen and hydrogen: N2(g) 3 H2gNH3(g) is an exothermic reaction: when 10.0 g of ammonia are produced in a bomb calorimeter, the temperature rises 3.92°C Determine the internal energy change (kJ mol-1) of this reaction. Take Ceal 3.07 kJ/oC h.s TARIS WTH THD.OR
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