G0 = H0 - TS0
H0 = -92.38 kJ/mol
S0 = -198.2 J/mol .K = - 0.1982 KJ/mol
T = 50.000C = 323 K
G0 = - 92.38 - 323 (- 0.1982)
G0 = - 28.36 KJ/mol
Hydrogen reacts with nitrogen to form ammonia (NH) according to the reaction 3 H lol Nyla)...
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
4. Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3H2(g) + N2(g) + 2NH3(g) The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AGⓇ at 25°C. Show work
From AHⓇ and AS 11. Hydrogen reacts with nitrogen to form ammonia (NH) according to the reaction 3H:(g) +Nz() 5 2NH,(g) The value of Alºis -92.38 kJ/mol, and that of AS is -198.2 J/mol K. Determine AG at 25°C. a. +5.897 x 109 kJ/mol d. -16,66 kJ/mol b. +297.8 kJ/mol +49.5 kJ/mol c.-33.32 kJ/mol Free Energy, Entropy, Enthalpy 12. A reaction with a low enthalpy of reaction value is not spontaneous at low temperature but becomes spontaneous at high temperature....
9. When nitrogen gas reacts with hydrogen gas to form ammonia, 92.38 kJ of heat are givern off for each mole of nitrogen gas consumed, under constant pressure and standard conditions. What is the correct value for the standard enthalpy of reaction in the thermo- chemical equation below when 0.750 mol of hydrogen reacts? N2(g) + 3H2(s) → 2 NH3(g) 10. How many grams of copper can be cooled from 50.0 oC to 32.3 oC by the heat gain by...
< Question 3 of 3 > Ammonia, NH, reacts with oxygen to form nitrogen gas and water. 4NH, (aq) + 30,(g) + 2N (8) + 6 H,0(1) If 2.45 g of NH, reacts with 3.68 g of O, and produces 0.850 L of N, at 295 K and 1.00 atm, which reactant is limiting? O NH3(aq) O 02(8) What is the percent yield of the reaction? percent yield: 55.7
Question 3 of 3 > Ammonia, NH), reacts with oxygen to form nitrogen gas and water. 4NH, (aq) + 30,(E) — 2N,(s) + 6H20(1) If 3.45 g of NH, reacts with 5.18 g of O, and produces 0.450 L of N, at 295 K and 1.00 atm, which reactant is limiting? - NH (0) 0,(8) What is the percent yield of the reaction? percent yield: 29.14
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3(g) NOTE: Throughout this tutorial use molar masses expressed to five significant figures. How many molecules (not moles) of NH3 are produced from 4.21×10−4 g of H2?
Solving moles-to-moles limiting reactant problems Nitrogen (N2) gas and hydrogen (H) gas react to form ammonia (NH) gas. Suppose you have 9.0 mol of N, and 1.0 mol of H, in a reactor. What would be the limiting reactant? Enter its chemical formula below.
1. Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation: 3 H2(g) + N2(g) → 2 NH3(2) - How many grams of H2 are needed to produce 14.43 g of NH3? 2. When propane (C2H8) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is... CzHz (g) + O2(g) → CO2(g) + H2O(g) This type of reaction is referred to as a complete...
Hint Resources Check Answer Question 3 of 3 Ammonia, NH, reacts with oxygen to form nitrogen gas and water 3 4 NH (aq)+30,(e) 2N,() +6H,0) If 2.75 g of NH, reacts with 4.13 g of O, and produces 0.850 L of N, at 295 K and 1.00 atm, which reactant is limiting? O 0,(g) O NH, (aq) What is the percent yield of the reaction? percent yield: