Calculate the mass of carbon dioxide produced from complete combustion of 16.6 g of octane, C8H18, in the following reaction. C8
H18 O2 --> CO2 H2O (unbalanced)
A. 51.2 g CO2
B. 102 g CO2
C. 57.6 g CO2
D. 0.799 g CO2
E. 1.163 g CO2
A. 51.2 g CO2
B. 102 g CO2
C. 57.6 g CO2
D. 0.799 g CO2
E. 1.163 g CO2
1 answer:
Answer:
51.2g of CO2
Explanation:
The first step is to balance the reaction equation as shown in the solution attached. Without balancing the reaction equation, one can never obtain the correct answer! Then obtain the masses of octane reacted and carbon dioxide produced from the stoichiometric equation. After that, we now compare it with what is given as shown in the image attached.
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<u>Answer:</u> The pH of acid solution is 4.58
<u>Explanation:</u>
To calculate the number of moles for given molarity, we use the equation:
.....(1)
- <u>For KOH:</u>
Molarity of KOH solution = 1.1000 M
Volume of solution = 41.04 mL
Putting values in equation 1, we get:
- <u>For propanoic acid:</u>
Molarity of propanoic acid solution = 0.6100 M
Volume of solution = 224.9 mL
Putting values in equation 1, we get:
The chemical reaction for propanoic acid and KOH follows the equation:
<u>Initial:</u> 0.1372 0.04514
<u>Final:</u> 0.09206 - 0.04514
Total volume of solution = [224.9 + 41.04] mL = 265.94 mL = 0.26594 L (Conversion factor: 1 L = 1000 mL)
To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:
We are given:
= negative logarithm of acid dissociation constant of propanoic acid = 4.89
pH = ?
Putting values in above equation, we get:
Hence, the pH of acid solution is 4.58