Using the formula CO2(g)+4H2(g)→CH4(g)+2H2O(g)   How many moles of methane are produced when 71.1 molesmoles of carbon dioxide gas react with excess hydrogen gas?

If 0.460 mol of liquid CS2 and 0.500 mol of gaseous O2 are reacted stoichiometrically according to the balanced equation, how many moles of gaseous CO2are produced? CS2(l) + 3O2(g) → CO2(g) + 2SO2(g) Molar Mass (g/mol) CS2 76.143 O2 31.998 CO2 44.009 Density (g/mL) CS2 1.26         Molar Volume (L) 22.4 at STP Gas Constant(L.atm.mol-1.K-1) 0.0821

The combustion of propane occurs through the following chemical reaction. C 3 H 8 ( g ) + 5 O 2 ( g ) ⟶ 3 C O 2 ( g ) + 4 H 2 O ( g ) How many grams of CO2 can be made by reacting 8.896 grams of oxygen gas?

Nitric Oxide can be made from the oxidation of ammonia as shown below. A reaction between 8.5 g of NH3 and 25.0 g of O₂ produces 12.0 g of NO. What is the percent yield for this reaction? 4 NH3(g) + 5O₂(g) → 4 NO(g) + 6 H₂O(g) Molar masses (in g mol-¹): NH3 17.034, 0₂ 32.00, NO 30.01, H₂O 18.016

When propane (C3Hg) reacts with oxygen, carbon dioxide and water are produced. The balanced equation for this reaction is C3 Hs (g) + 502 (g) → 3CO2(g) + 4H2O(g) If 10 moles of oxygen react, The reaction consumes moles of propane (C3H8). The reaction produces moles of carbon dioxide and moles of water.

Determine the mass in grams of CO₂ that are produced by the complete reaction of 0.05090 moles of C₇H₈ (toluene) according to the following combustion reaction: C₇H₈(l)+ 9 O₂(g) → 7 CO₂(g) + 4 H₂O(g)

Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction.   NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g)  What is the theoretical yield of solid copper that should form when 18.1 g of NH3 is reacted with 90.4 g of CuO?

STARTING AMOUNT X This question will walk you through the steps of determining which reactant is limiting based on a balanced chemical equation. Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in moles CO₂ from the complete combustion of 29.3 grams CH4 according to the following balanced chemical equation: 1 CH4(g) + 2 O₂(g) → 1 CO₂(g) + 2 H₂O(1) 56.2 ADD FACTOR x( ) 1.83 g CO₂ 0.547 44.01 1 29.3 2 ANSWER 16.05 0.915 0.666 g/mol CO₂ mol CO₂ g/mol CH4 mol CH4 RESET 5 18.02 g CH₂ 16.00