Consider the following equation, which represents the combustion of hydrogen sulfide. 2H2S(g)+3O2(g)→2SO2(g)+2H2O(g)   a) What volume, in liters, of SO2 is formed when 137 L of H2S(g) is burned? Assume that both gases are measured under the same conditions. b) What volume, in liters, of O2(g) is required to form 28 L of H2O(g)? Assume that both gases are measured under the same conditions.

Calculate the number of moles of water produced when 3.3 mol of Cu(NO3)2 are formed in the reaction.

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH₂ (g) + 20₂(g) → HNO3(g) + H₂O (g) Suppose the yield of the first step is 61.% and the yield of the second step is 77.%. Calculate the mass of nitrogen required to make 10.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 Explanation Check. ☐ x10 8 X 09 0.0 S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |

If you wanted to produce 4 moles of SO3 gas, how many moles of SO2 would you need to react? (Assume an unlimited supply of O2 gas.) 2 SO₂ (g) + O₂(g) →2 SO, (g)

A sample of 48.7 g of tetraphosphorous decoxide (P₂O₁0) reacts with 84.6 g of water to produce phosphoric acid (H₂PO4) according to the following balanced equation. PAO10 + 6H₂O4 H₂PO4 Determine the limiting reactant for the reaction. OH₂O O H₂PO4 OP40 10 Calculate the mass of H₂PO4 produced in the reaction. mass of H₂PO4:

Ammonia (NH3) is an important compountd is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) +H2(g) = NH;(g) When 1.20 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) mol b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places) mol c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) Activate W mol d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) 10:09 Links 18°C 1O 23-Nov-21

A 6.79 g sample of NH, gas and a 6.79 g sample of HCl gas are mixed in a 1.50 L flask at 25 °C. < EFeedback You have not correctly determined the mass of NH,Cl formed. Identify the limiting reagent. Convert the given mass of the limiting reagent to the mass of NH,Cl using the NH; mole ratio from the balanced chemical HCI equation and the molar masses for both NH,CI the limiting reagent and the NH,Cl as conversion factors. How many grams of NH,Cl will be formed by this reaction? 0.273 mass: Incorrect What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH,Cl produced by the reaction. P = 3.42

Calcium hydride reacts with water to produce hydrogen gas according to the following reaction: CaH2(s)  + 2 H2O(l)  ----> 2H2(g)  +  Ca(OH)2(aq) This reaction is used to generate hydrogen gas to inflate air bags in cars and life rafts on boats and for similar uses where a simple compact means of hydrogen generation is necessary.  Assuming complete reaction with water, how many grams of calcium hydride are required to fill a raft to a total pressure of 2.0 atm at 25oC if the volume of the raft is 1,000 L?

Before the use of CFCs, sulfur dioxide was used as a refrigerant.  A sample of sulfur dioxide undergoes a simple decomposition reaction as follows: 8 SO2(g) --> S8(s)  +  8 O2(g) Calculate the number of moles of oxygen gas produced in addition to the production of 1.18 mol of sulfur.

Carborundum (silicon carbide), SiC, is a very hard material used as an abrasive on sandpaper and in other applications. It is prepared by the reaction of pure sand, SiO2, with carbon at high temperature. Carbon monoxide, CO, is the other product of this reaction. (a) Write the balanced equation for this reaction. (Omit states - of - matter from your answer. Use the lowest possible whole number coefficients.) chemPadHelp (b) Calculate how many kilograms of SiO2 are required to produce 3.14 kg of SIC.