H H | 29 The compound C6H5C-N-N=CC6H5 is produced by the reaction of an excess of...
14. A compound contains C, H and N atoms. When burned in an air with excess oxygen, a 0.312 g sample produced 0.458 g CO2 and 0.374 g H2O. The nitrogen content of a 0.486 g sample is converted to 0.226 g N2. What is the empirical formula of the compound? -5 3.89 X10 mcle A) CHAN В) С2НаN C) CH4N2 D) C3H4N2 E) C3H4N 7.99 I65 mol4 1,50 molo
54) Dissolving benzaldehyde in methyl alcohol establishes an equilibrium with what compound(s)? OH a) CHECHOCHZ b) CoH5COCH3 c) C6H5C(OCH3)3 OH d) CoH;CHOCH3 and CoH3COCH3 07 e) CoH5COCH3 and C6H5C(OCH3)3
Hydrogen gas (H 2 ) and nitrogen gas (N 2 ) combined through the Habes process to produce ammonia gas (NH 3 ) This industrial process occurs at extremely high temperatures and pressures. 3H 2 (g)+N 2 (g) 2NH 3 (g) If 50.9 H 2 combined with excess nitrogen gas and the pressure and temperature are maintained at 201 atm and 460.0 C throughout the reaction, how many grams of ammonia gas will be produced? 3080 113 g g 1930...
hydrazine N2H4 reacts with oxygen to form nitrogen gas and water Hydrazine, N, H, reacts with oxygen to form nitrogen gas and water. N,H, (aq) +0,6) N,(g) + 2 H2O(1) If 2.45 g of N, H, reacts with excess oxygen and produces 0.950 L of N,, at 295 K and 1.00 atm, what is the percent yield of the reaction? percent yield:
Hydrazine, N, H, reacts with oxygen to form nitrogen gas and water. N, H(aq) + O2(g) —N,() + 2 H2O(1) If 2.35 g of N, H, reacts with excess oxygen and produces 0.850 L of N,, at 295 K and 1.00 atm, what is the percent yield of the reaction? percent yield:
f a compound consisting of carbon, hydrogen, oxygen, nitrogen, and sulfur was combusted in excess oxygen. This produced 2.20 g Co2 and 1.20 g H,O. A second sample of this compound with a mass of 4.86 g produced 3.19 g SO,. A third sample of this compound with a mass of 8.86 g produced 4.57 g HNO,. Determine the empirical formula of the compound. Enter the correct subscripts on the given chemical formula. empirical formula: CHNSO f a compound consisting...
Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) + 2NH3(g) Calculate the mass of ammonia produced when 33.0 g of nitrogen react with 11.2 g of hydrogen. Which is the excess reactant and how much of it will be left over when the reaction is complete? o hydrogen nitrogen
Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) Calculate the mass of ammonia produced when 32.0 g of nitrogen react with 13.5 g of hydrogen. ___________NH3 Which is the excess reactant and how much of it will be left over when the reaction is complete? hydrogen or nitrogen ________ g
d. The "complete" mechanism of the reaction is shown below (actually, I've simplified it just a bit). Hydrazine (N2Ha) is an intermediate in the reaction pathway, and the reaction consists of two elementary steps. Draw a reaction coordinate diagram that represents the key features of the reaction, including the relative energies of the reactants and products 2 H2 (g)+ N2g) N,H4 (g) (Slow) H2 (g) + N,H82 NH, (g) e. Write the instantaneous rate law for this reaction. f. 100.0...
How many moles of NH3 can be produced from 21.0 mol of H, and excess N? C AR vaur anexer numerically in moles. How many grams of NH, can be produced from 3.18 mol of N, and excess H,