If 7.4 moles of carbon dioxide is produced in this reaction, how many moles of oxygen gas would be needed?
1 answer:
Answer:
11.6 mol O₂
Explanation:
- C₇H₁₆ + 11 O₂ → 7 CO₂ + 8 H₂O
In order to solve this problem we need to <u>convert moles of carbon dioxide (CO₂) into moles of oxygen gas (O₂)</u>. To do so we'll use a conversion factor containing the <em>stoichiometric coefficients</em> of the balanced reaction:
- 7.4 mol CO₂ *
= 11.6 mol O₂
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Answer:
TS (total solid, mg/L) = 57,174 mg/L
VS (volatile solid, mg/L) = 24,088 mg/L
Explanation:
First step to solve this problem is to know data and questions:
Data:
Sample volume = 50 mL
Sample weight = 50.1 g
P1 (weight empty crucible) = 17.1234 g
P2 (weight after drying a 103º in oven) = 19.9821 g
P3 (weight after incinatrion 550º) = 18.7777 g
Questions:
TS = ?
VS = ?
Formula:
We need to use formulas to calculate total solid (TS) and volatile solid (VS), these are:
We have to transform mL to L so we will divide mL by 1,000 the sample volume:
In the formula the value of 1,000 results by the convertion factor to transform grams to miligrams (we have to multiplie by 1,000)
Now we need to replace data on previous formulas and we will get TS and VS expressed in mg/L:
We divide TS and VS formula by sample volume because the exercise is asking us to express the results in mg/L.