Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 460kJ of heat. C(s)+O2(g)❝CO2(g)ΝH❝rxn=❝393.5kJ
C + O2 --> CO2 delta H rxn = -393.5
First, they gave you that the enthalpy of reaction is -393.5 kJ/mole (those are the units that should have been included). The amount of material to give you 520 kJ is
Moles carbon = 460 kJ/(393.5 kJ/mole) = 1.168 moles
Moles CO2 = moles C = 1.32 moles
Mass CO2 = 1.168 moles * 44.01 g/mole = 51.44g
Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 460kJ of heat. C(s)+O...
Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 450 kJ of heat. C(s)+O2(g)→CO2(g)ΔH∘rxn=−393.5kJ
Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 4.50×10^2 kJ of heat. C(s)+O2(g)→CO2(g) ΔrH∘= −393.5kJ mol−1
Determine the mass of CO2produced by burning enough carbon (in the form of charcoal) to produce 450 kJ of heat. C(s)+O2(g)→CO2(g)ΔH∘rxn=−393.5kJ
Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon to produce 5.00 x 102 kJ of heat. C(s) + O2(g) = CO2(g) DH = -393.5 kJ
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A) A silver block, initially at 55.4 ∘C, is submerged into 100.0 g of water at 25.3 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.8 ∘C. What is the mass of the silver block? B) Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.50×102kJ of heat? The balanced chemical equation is as follows: C(s)+O2(g)→CO2(g),ΔH∘rxn=−393.5kJ
Calculate the heat change, in kJ, if 8.7395x1012 ng of carbon dioxide were produced in the following reaction: C(s) + O2(g) CO2(g) AH = -393.5 kJ/mol q=C MAT
Many power plants produce energy by burning carbon-based fuels, which also produces carbon dioxide. Carbon dioxide is a greenhouse gas, so over-production can have negative effects on the environment. Use enthalpy of formation data to calculate the number of moles of CO2(g) produced per megajoule of heat released from the combustion of each fuel under standard conditions (1 atm and 25 �C). Each must be in mol * MJ^-1 (a) coal, C(s, graphite) (b) natural gas, CH4(g); (c) propane, C3H8(g);...
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