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The total number of grams of CO2 that are produced when 4 grams of C are added to 10.67 grams of O2?
Wiki User
∙ 14y ago
13.3g
C + O2 = CO2
m(C)=4g => n(C)=4/12=0,333mol
m(O2)=10.67g => n(O2)=10.67/28=0,381mol
we have excess of oxigen
n(CO2)=n(C)=0,333
m(CO2)=0.333*40=13.3g
Wiki User
∙ 14y ago
To calculate the total grams of CO2 produced, first determine the moles of each element by dividing the mass by the molar mass. Then identify the limiting reactant (the one that produces the least moles of CO2) and use the stoichiometry of the balanced chemical equation to find the moles of CO2 produced from it. Finally, convert the moles of CO2 to grams using the molar mass of CO2.
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What is the balanced equation for The total number of grams of CO2 that are produced when 4 grams of C are added to 10.67 grams of O2?
The balanced equation is: 2C + O2 -> 2CO2. First, determine the moles of C and O2: 4g C / 12 g/mol = 0.33 mol C and 10.67g O2 / 32 g/mol = 0.33 mol O2. From the balanced equation, 2 moles of C produces 2 moles of CO2, so 0.33 mol C will produce 0.33 mol CO2. Since CO2 has a molar mass of 44 g/mol, the total grams of CO2 produced will be: 0.33 mol CO2 x 44 g/mol = 14.52 grams of CO2.
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What is the balanced equation for The total number of grams of CO2 that are produced when 4 grams of C are added to 10.67 grams of O2?
The balanced equation is: 2C + O2 -> 2CO2. First, determine the moles of C and O2: 4g C / 12 g/mol = 0.33 mol C and 10.67g O2 / 32 g/mol = 0.33 mol O2. From the balanced equation, 2 moles of C produces 2 moles of CO2, so 0.33 mol C will produce 0.33 mol CO2. Since CO2 has a molar mass of 44 g/mol, the total grams of CO2 produced will be: 0.33 mol CO2 x 44 g/mol = 14.52 grams of CO2.
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