Answer:
4.5 moles of carbon dioxide
Explanation:
Given parameters:
Mass of CH₄ = 72g
Unknown:
number of moles of CO₂ produced = ?
Solution:
To solve this problem, let us write the reaction equation first;
CH₄ + 2O₂ → CO₂ + 2H₂O
Now we know that O₂ is in excess and CH₄ is the limiting reactant that will determine the extent of the reaction.
Let us find the number of moles of CH₄ ;
Number of moles = 
molar mass of CH₄ = 12 + 4 = 16g/mol
Number of moles = 
= 4.5moles
From the reaction equation;
1 mole of methane produced 1 mole of carbon dioxide
4.5 moles of methane will produce 4.5 moles of carbon dioxide
Answer:
The solution has 11.4 μg protein
Explanation:
Hi there!
The corrected absorbance will be the measured absorbance minus the absorbance of the blank that is a solution without protein.
Then, the corrected absorbance will be:
0.276 - 0.061 = 0.215
Now, using the equation of the calibration curve, we can obtain the quantity of protein present in the solution:
0.215 = 0.0182x + 0.007
(0.215 - 0.007) / 0.0182 = x
x = 11.4 μg
The solution has 11.4 μg protein
Missing question:
Suppose Gabor, a scuba diver, is at a depth of 15 m. Assume that:
1. The air pressure in his air tract is the same as the net water pressure at this depth. This prevents water from coming in through his nose.
2. The temperature of the air is constant (body temperature).
3. The air acts as an ideal gas.
4. Salt water has an average density of around 1.03 g/cm^3, which translates to an increase in pressure of 1.00 atm for every 10.0 m of depth below the surface. Therefore, for example, at 10.0 m, the net pressure is 2.00 atm.
T = 37°C = 310 K.
p₁ = 2,5 atm = 253,313 kPa.
p₂ = 1 atm = 101,325 kPa.
Ideal gas law: p·V = n·R·T.
n₁ = 253,313 kPa · 6 L ÷ 8,31 J/mol·K · 310 K.
n₁ = 0,589 mol.
n₂ = 101,325 kPa · 6 L ÷ 8,31 J/mol·K · 310 K.
n₂ = 0,2356 mol.
Δn = 0,589 mol - 0,2356 mol = 0,3534 mol.
