Answer:
Approximately 5.05 g of CO2 are used when 6.50 g of O2 are produced.
Explanation:
The answer to this question is the implication that the production of 6.5g of O2 requires 5g-6g CO2, since it is 63% oxygen by mass and 37% carbon dioxide by mass (not including water vapor). This would mean that 4g-5g CO2 productions could be expected to yield 2.25 or so grams oxygen for each gram CO2 produced, depending on how low the temperature was at which the reaction took place (a product like dry ice produces only cold enough to use 1/16th its volume in volume rather than 1/200th).
Are you looking for the definition or answer? Since nomenclature is just definition by name or giving a specific name; the overall answer should be Carbon Dioxide.
Answer:
See explanation
Explanation:
Total number of moles of gases in the mixture; 0.70 + 0.25 + 0.05 = 1 mole
Partial pressure= mole fraction of gas × total pressure
Mole fraction of hydrogen = 0.7/1 × 2.6 = 1.82 atm
Mole fraction of CO2 = 0.25/1 × 2.6 = 0.65 atm
Mole fraction of CO= 0.05/1 × 2.6 = 0.13 atm
<em>9. A</em>
<em>10. B</em>
<em>11. B</em>
<em>12. C</em>
<em>13. D</em>
<em>14. C
</em>
I hope this helped! (: