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Suppose, for example, 8.75 g of propane (C3H8) react with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O). How many grams of water are produced?
Grams of water produced=3.72g
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methane(CH⁴) burns in oxygen to produce carbon dioxide and water vapor , what is the number of(CH²) MOLECULES produced when 3.2 L of oxygen are comsumed?
Methane(CH4) burns in oxygen to produce carbon dioxide and water vapor.What is the number of (CO2) molecules produced when 3.2 L of oxygen are comsumed?Solution:Calculate the moles of oxygen gas...
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Construct a balanced chemical equation for the conversion of methane gas and oxygen into carbon dioxide and water.
CH4 + 2O2 = 2H2O + CO2
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The combustion of methane gas is described by the equation CH4+2O2→CO2+2H2O.
What volume of oxygen is needed at STP to combust 4.7 L methane?
How much carbon dioxide will be formed?
CH4+2O2→CO2+2H2O V(O_2 ):V(CH_4 )=2:1 V(O_2)=V(CH_4 )×2=4.7×2=9.4 L V(CO_2 ):V(CH_4 )=1:1 V(CO_2)=V(CH_4 )=4.7 L Answer: V(O2) = 9.4 L, V(CO2) = 4.7 L.
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A 40.8 mol sample of methane gas CH4(g) is placed in a 1020 L container at 298 K. What is the pressure, in atm of the methane gas?
ollowing the Ideal gas law: pV=nRT where R is gas constant and equal to 0.0821 L·atm·K-1·mol-1 For this case, pressure in atm have been equal to: p=nRTV=40.8 (mol)∙0.0821 (L∙atm∙K-1∙mol-1)∙298 (K)/...
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Methane is heteroatomic- containing the elements carbon and hydrogen. Each molecule of methane is pentatomic, and contains only one atom of carbon.
Solution: Methane is heteroatomic- containing the elements carbon and hydrogen. Each molecule of methane is pentatomic, and contains only one atom of carbon – True. CH4.
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A 40.8 mol sample of methane gas CH4 is places in a 1020 L container at 298K.
What is the pressure, in atm of the methane gas?
Use the ideal gas law. From original equation PV=nRT there is P=nRT/V, R=8.31441J/(K∙mol)=0.08206(L∙atm)/(K∙mol), i.e. P (atm) = (40.8 mol*0.08206(L∙atm)/(K∙mol)*298K)/1020 L = 0.9782 atm Answer: 0.9782 atm
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Ten grams of calcium carbonate was produced when carbon dioxide was added to lime water (calcium hydroxide in solution). What volume of carbon dioxide at STP was needed
CO2 + Ca(OH)2 = CaCO3 + H2Om(CaCO3) = 10.0 g(10 g CaCO3 / 1)(1 mol / 100.1 g)(1 mol CO2 / 1 mol CaCO3)(22.4 L STP / 1 mol) = 2.24 L CO2 STP
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How many moles of oxygen are produced when 756 grams of lead 11 oxide are formed
Find the mass of nitrogen dioxide that forms with 0.58 moles of oxygen
1) 2 Pb + O2 = 2 PbOthe amount of PbO is 756 g / 223.2 g/mole = 3.38 mole, it is twice of moles of O2, i.e.the amount of...
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The complete combustion of heptane (C7H16) in oxygen produces carbon dioxide and water.
If I had 4.75g of heptane and combusted this to completion, how many grams of carbon dioxide would I produce?
100 gm of heptane will form 308 gm of carbon dioxide.So 4.75 gm of heptane will form 14.63 gm of carbon dioxide14.63 gm of CO2 will be produced
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