Answer: The mass of [tex]CO_2[/tex] produced will be 8.228 g.
Explanation:
We need to find the mass of carbon dioxide produced when 150 kJ of heat is released.
For the given chemical reaction:
[tex]CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g);\Delta H^o_{rxn}=-802.3kJ[/tex]
By Stoichiometry of the reaction:
802.3 kJ of energy is released when 1 mole of carbon dioxide is produced.
So, 150 kJ of energy will be release when = [tex]\frac{1}{802.3}\times 150=0.187mol[/tex] of carbon dioxide is produced.
To calculate the mass of carbon dioxide, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Moles of carbon dioxide gas = 0.187 mol
Molar mass of carbon dioxide gas = 44 g/mol
Putting values in above equation, we get:
[tex]0.187mol=\frac{\text{Mass of carbon dioxide gas}}{44g/mol}\\\\\text{Mass of carbon dioxide gas}=8.228g[/tex]
Hence, the mass of [tex]CO_2[/tex] produced will be 8.228 g.
The mass of CO₂ produced by burning enough methane to produce 1.50×10² KJ of heat is 8.23 g
Balanced equation
CH₄ + 2O₂ —> CO₂ + 2H₂O ΔHrxn = −802.3 KJ
From the balanced equation above,
802.3 KJ of heat produced 1 mole of CO₂.
Therefore,
1.50×10² KJ of heat will produce = 1.50×10² / 802.3 = 0.187 mole of CO₂
Mass = mole × molar mass
Mass of CO₂ = 0.187 × 44
Mass of CO₂ = 8.23 g
Learn more about stoichiometry:
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