If 0.245 mol of H2SO4(g) reacts with excess NH3(g) at 75°C for the following reaction,
2NH3(g) + H2SO4(g) → (NH4)2SO4(s)
what is the work done in terms of the system?
If 0.245 mol of H2SO4(g) reacts with excess NH3(g) at 75°C for the following reaction, 2NH3(g)...
If 0.685 mol of NH3(g) reacts with excess HCl(g) at 50°C for the following reaction, NH3(g) + HCl(g) → NH4Cl(s) what is the work done in terms of the system?
If 0.685 mol of NH3(g) reacts with excess HCI(g) at 50°C for the following reaction, NH3(g) HCl(g) NH4CI(s) what is the work done in terms of the system? +3.68 kJ -1.84 kJ +1.84 kJ -3.68 kJ
Question 10 (1 point) If 0.685 mol of NH3(g) reacts with excess HCl(g) at 50°C for the following reaction, NH3(g)+ HCl(g)NH4CI(s) what is the work done in terms of the system? +1.84 kJ O-1.84 kJ O-3.68 kJ +3.68 kJ
If 58 moles of NH3 are combined with 32 moles of
sulfuric acid, what is the limiting reactant and how much of the
excess reactant is left over?
2 NH3 + H2SO4
(NH4)2SO4
A) H2SO4, 29 mol
B) NH3, 1.0 mol
C) NH3 29 mol
D) NH3, 3.0 mol
E) H2SO4, 3.0 mol
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
Consider the balanced equation for the following reaction: 3H2O(l) + Mg3N2(aq) → 3MgO(s) + 2NH3(g) If 6.60 moles of H2O(l) reacts with an excess of Mg3N2(aq), determine the theoretical yield of NH3(g).
3H2(g)+N2(g)→2NH3(g) a. How many moles of NH3 can be produced from 13.5 mol of H2 and excess N2? b. How many grams of NH3 can be produced from 4.90 mol of N2 and excess H2. c. How many grams of H2 are needed to produce 12.74 g of NH3? d. How many molecules (not moles) of NH3 are produced from 1.05×10−4 g of H2?
When ammonia (NH3) reacts with fluorine (F2), the products are dinitrogen tetrafluoride and hydrogen fluoride. 2NH3(g)+5F2(g)→N2F4(g)+6HF(g) How many moles of NH3 are needed to produce 3.00 mol of HF? How many moles of F2 are needed to produce 3.00 mol of HF? How many grams of F2 are required to react with 26.5 g of NH3? How many grams of N2F4 can be produced when 3.55 g of NH3 reacts?
Give the data in table below,
Hrxn for the reaction.
NH3(aq)+H2SO4(aq)HSO4-(aq)+NH4+(aq)
Compound / Hf
(kj/mol)
NH3= -80.29
H2SO4= -909.3
NH4+= -132.5
HSO4- = -212.08
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g)?H°f (kJ mol-1)S° (J K-1 mol-1)NH3(g)-46193O2(g)0205CH4(g)-75186HCN(g)135.1202H2O(g)-242189The above reaction is used in the industrial production of hydrogen cyanide. (The tabulated values ?H°fand S° are for 25°C. For the purposes of this question assume that ?H° and ?S° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)?H° is -939.8?S° is 165Calculate ?G° at 1005°C, for this equation.Are the following statements about this process True...