When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. C (s) + O2 (g) → CO2 (g) However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. 2C (s) + O2 (g) → 2CO2 (g) What mass of each product is expected when a 5.00-g sample of pure carbon is burned under each of these conditions?

Consider the following: 4NH3 + 5O2 → 4NO + 6H2O In an experiment, 5.42 g of NH3 are allowed to react with 7.26 g of O2. How many grams of NO are formed?

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: N2(g) + 3H2(9) → 2NH3(g) 1. What is the maximum mass of ammonia that can be produced from a mixture of 191.3 g of N2 and 46.25 g of H2? 2. Which element would be completely consumed? (enter nitrogen or hydrogen) 3. What mass of the starting material would remain unreacted? Submit Answer Tries 0/10

For the reaction CH4 (g) + Cl2 (9) → CH3 Cl (g) + HCl (g) When 41.6 g of CHĄ and 84.0 g of Cl, reacts completely, what is the mass of HCl that could be produced? Molar mass: CH4 = 16.05 g mol-1; Cl2 = 70.90 g mol-1; HCI = 36.46 g mol-1 O 43.2 g O 94.5 g O 191. g O 18.3 g O 21.4 g

Coal is a leading source of energy for the world. While coal is primarily composed of carbon and hydrogen, a small amount of sulfur is also present. This leads to the production of pollutants such as sulfur dioxide (SO2) through the following reaction: S(s)+O2(g)→SO2(g) A sample of coal was found to contain 1.35% sulfur by mass. If 1,250 kg of this coal were burned, what mass of sulfur dioxide could theoretically be formed (in kg)?

Barium hydride reacts with water to produce barium hydroxide and hydrogen gas. BaH₂ (s) + 2 H₂O(1)→ Ba(OH)2 (aq) + H₂(g) If 6.389 g BaH2 is combined with 64.000 g H₂O, the reaction proceeds until all the BaH₂ is consumed. The hydrogen gas escapes to the environment, and the final weight of the flask is 70.204 g. The remaining water is evaporated, leaving 7.856 g Ba(OH)2. What mass of water is consumed in the reaction? g H₂O BO esc :0 F1 2 1086 TeTWE F2 # OCT 3 3 80 F3 $ 4 F4 R 65 % F5 T COMING MacBook Pro < 6 F6 Y & A 7 aa F7 * 00 U 8 DII F8 tv A S I F9 2 S F10 0 0 Save and Exit a F11

Consider the decomposition of ammonia: 2 NH3 (g) → 3H2 (g) + N2 (g). If you start with 425g of NH3, how many grams of H2 and N2 can be produced?

SO2(g) + H2O(l) → H2SO3(g) Given an initial mass of 14.12 g SO2, an excess of H2O, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H2SO3 produced by the reaction.

Acrylonitrile (C3H3N) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction. 2C3He (9) + 2 NH3 (9) + 302 (9) → 2C,H,N(g) + 6H2O(g) If 20.0 g C3 H6 , 15.0 g O2, and 10.0 g NH3 are reacted, what mass of acrylonitrile can be produced, assuming 100% yield? Mass = g

Chemistry Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 20.0 g N2O4 and 25.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol. Show calculations               N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)