4NH3(g) + 7O2(g) ------ 4NO2(g) + 6H2O(g)
Molar mass of NH3 = 14 + 3 * 1 = 17 gm/mol
Number of moles of ammonia = 43.9/17 = 2.582 moles
4 moles of NH3 will give 4 moles of NO2
Hence moles of NO2 formed = 2.582 moles
Molar mass of NO2 = 14 + 2 * 16 = 46 gm/mol
Mass of NO2 formed = 2.582 moles * 46 gm/mol
=> 118.788 gms
The combustion of ammonia in the presence of excess oxygen yields NO_2 and H_2O: 4 NH_3(g)+7O_2(g)...
43) The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4 NH3 (g)+702 (g) 4 NO2 (g)+6 H20 (g) The combustion of 14.4 g of ammonia consumes O541-80f oxygen A) 13.5 B) 47 D) 28.8 E) 94.6 6
The combustion of ethene in the presence of excess oxygen yields carbon dioxide and water: ΔS° values: C2H4(g) = 219.4J/K; O2 (g) = 205 J/K; CO2 (g) = 213.6 J/k; H2O (g) =69.91 J/K C2H4 (g) + 3O2 (g) --> 2CO2 (g) + 2H2O (l) This value of ΔS° for this reaction is _____ J/K mol A. -267.4 B. -140.9 C. -347.6 D. +347.6 E. +140.9
In the combustion of hydrogen in the presence of excess oxygen, if 5.85 g of molecular hydrogen (H2) are combusted, what mass of water (in g) will be produced? Report your answer to 2 decimal places and include units.
The combustion of liquid octane, C8H18, in the presence of gaseous oxygen yields carbon dioxide and liquid water. Write the balanced equation for the reaction, including physical states.
Question 5 Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al(s) + 302 (g) → 2A1203 (s) The maximum amount of A1203 that can be produced from 2.5 g of Al and 2.5 g of O2 is 5.0 ③ 4.7 3 9.4 * 5.3 * 7.4 Question 3 -/1 The combustion of ammonia in the presence of excess oxygen yields NO2 and H20: 4 NH3(g) + 7 02 (g) → 4NO2(g) + 6H20 (g)...
A 2.50 g sample of ethanol, C2H5OH, was combusted in the presence of excess oxygen in a bomb calorimeter containing 2.00 kg of water. The temperature of the water increased from 22.500oC to 27.845oC. The heat capacity of the calorimeter is 2520 J/oC and the specific heat capacity of water is 4.184 J/goC. Calculate the molar enthalpy of the combustion reaction in kJ/mol
4) If 300.0 g of butane were completely combusted in the presence of excess oxygen, what mass of CO2 would be produced?
Nitrogen monoxide is produced by combustion in an automobile engine. For the following reaction, 6.22 grams of nitrogen monoxide are mixed with excess oxygen gas. The reaction yields 7.45 grams of nitrogen dioxide. nitrogen monoxide (g) + oxygen (g) Right arrow nitrogen dioxide (g) What is the theoretical yield of nitrogen dioxide? grams What is the percent yield for this reaction? %
2. Combustion of 1.000 g of the compound that has carbon, oxygen and hydrogen yields 1.734 g CO, and 0.803 g H,O. In another experiment, 0.1067 g of the compound was dissolved in 23.6 g of water. This solution had a freezing point of -0.0914°C. What is the molecular formula of the compound?