Calculate ΔS°rxn (J/k) for 3NO2(g) + H2O(l)LaTeX: \longrightarrow⟶ NO(g) +2HNO3(l) C6H12O6(s) + 6O2(g) LaTeX: \longrightarrow⟶ 6
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Answer:
Explanation:
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In this case, the undergoing chemical reaction is:
Next, we identify the limiting reactant by computing the moles of magnesium oxide yielded by 3.86 g of magnesium and 155 mL of oxygen at the given conditions via their 2:1:2 mole ratios and the ideal gas equation:
It means that the limiting reactant is the oxygen as it yields the smallest amount of magnesium oxide. Next, we compute the mass of magnesium consumed the oxygen only:
Thus, the mass in excess is:
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Answer:
The molar mass of the protein is 12982.8 g/mol.
Explanation:
The osmptic pressure is given by:
π=MRT
Where,
M: is molarity of the solution
R: the ideal gas constant (0.0821 L·atm/mol·K)
T: the temperature in kelvins
Hence, we look for molarity:
= =5.584×10⁻³mol/l
As we have 2 ml of solution, we can get the moles quantity:
Moles of protein: 5.584×10⁻³×2ml=1.117×10⁻⁵mol
Finally, the moles quantity is the division between the mass of the protein and the molar mass of the protein, so:
Moles=Mass/Molar mass
Molar mass= Mass/Moles==12982.8 g/mol