Suppose 8.00 g of CH4 is allowed to burn in the presence of 15.30 g of...
Suppose 8.60 g of CH4 is allowed to burn in the presence of 16.40 g of oxygen. CH(9) +202 (9) →C02(g) + 2H20(9) How much (in grams) O, remains after the reaction is complete? og Previous Answers Correct Part 0 How much (in grams) CO2 remains after the reaction is complete? IVO AED 0 2 ? Submit Request Answer Part D Complete previous part(s)
Suppose 8.30 g of CH4 is allowed to burn in the presence of 15.70 g of oxygen. CH4(g) + 2O2(g) →CO2(g) + 2H2O(g) Part A How much (in grams) CH4 remains after the reaction is complete? IVO AQ R O 2 ?
Part A What mass of natural gas (CH) must you burn to emit 268 kJ of heat? CH4 (g) + 202 (g) + CO2(g) + 2H2O(g) AH = -802.3 kJ Express the mass in grams to three significant figures. O AL M O O ? Submit Request Answer
What mass of natural gas (CH4) must you burn to emit 259 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ Express the mass in grams to three significant figures.
Exactly 17.550 g of O2 is required to completely burn a 5.000 g mixture of CH4 and C2H2 yielding only CO2 and H2O. How many grams of C2H2 were in the original mixture? The combustion equations are: CH4(g) + 2 O2(g) ----> CO2(g) + 2 H2O(g) C2H2(g) + 5/2 O2(g) ----> 2 CO2(g) + H20(g)
An empty 3.70 L steel vessel is filled with 2.00 atm of CH4(g) and 8.00 atm of O2(g) at 300 ∘C. A spark causes the CH4 to burn completely, according to the equation: CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔH∘ = -802kJ 1. What is the final temperature inside the vessel after combustion, assuming that the steel vessel has a mass of 12.475 kg , the mixture of gases has an average molar heat capacity of 21J/(mol⋅∘C), and the heat capacity of steel is 0.499J/(g⋅∘C)?...
Part A If 8.6 g of CH4 and 5.0 g of O2 react, what is the mass, in grams, of H2O that is produced? CH (g)+202(g)CO2(g) +2H20(g) Express your answer with the appropriate units. HA m(H2O) = Value Units Submit Request Answer
1. What mass of natural gas (CH4) must you burn to emit 260 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔH∘rxn=−802.3kJ 2.Consider the following thermochemical equation for the combustion of acetone, C3H6OC3H6O, the main ingredient in nail polish remover: C3H6O(l)+4O2(g)→3CO2(g)+3H2O(g)ΔH∘rxn=−1790kJ If a bottle of nail polish remover contains 173 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL 3.Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When...
Consider the reaction CH4(g) + 202(g) = CO2(g) + 2H2O(l). If the standard free energy of the reaction is -817.8 kJ, what is the free energy (in kJ) of a reaction vessel containing 1.2 M CH4,0.58 M 02, and 4.2 M CO2, at 298K? Don't include units in the answer.
(#1 continued) 16.05 g mole 44.01 g mole CH4 202-CO2 2 H:0+802.3 k 200 gmole15.02 gme c. How many grams of water are produced by the complete combustion of 237.00 g of methane with 500.00 g of oxygen? d. What is the limiting reactant? e. what is the excess reactant? f. Refer back to part (c) When s used up, the reaction stops. H:O CH4 02