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Alexxx [7]
3 years ago
5

When she carried out her experiment, Tanya used three small vials of the

Chemistry
1 answer:
sleet_krkn [62]3 years ago
8 0
It’s a I hope it rightgood luck
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Consider the equation for the formation of water.
Juli2301 [7.4K]

The theoretical yield is 160 g H₂O.

<em>Moles of H₂</em> = 18 g H₂ × (1 mol H₂/2.016 g H₂) = 8.93 mol H₂

<em>Moles of H₂O</em> = 8.93 mol H₂O × (2 mol H₂O/2 mol H₂) = 8.93 mol H₂O

<em>Theoretical yield</em> of H₂O = 8.93 mol H₂O × (18.02 g H₂O/1 mol H₂) = 160 g H₂O

6 0
3 years ago
Na2SO4 is dissolved in water to make 450mL of a 0.2250 M solution. What is the molar mass of Na2SO4?
Alisiya [41]

Answer:

mass Na2SO4 = 14.3816 g

Explanation:

sln Na2SO4:

∴ V = 450 mL

∴ <em>C </em>=<em> </em>0.2250 mol/L

∴ Mw ≡ 142.04 g/mol.....  from literature

⇒ mol Na2SO4 = (0.2250 mol/L)(0.450 L) = 0.10125 mol

⇒ mass Na2SO4 = (0.10125 mol)(142.04 g/mol) = 14.3816 g

3 0
3 years ago
Fructose-1-P is hydrolyzed according to: Fructose-1-P + H2O → Fructose + Pi If a 0.2 M aqueous solution of Froctose-1-P is allow
aalyn [17]

Answer:

\Delta G^{\circ}=-15902 J/mol

Explanation:

In this problem we only have information of the equilibrium, so we need to find a expression of the free energy in function of the constant of equilireium (Keq):

\Delta G^{\circ}=-R*T*ln(K_{eq})

Being Keq:

K_{eq}=\frac{[fructose][Pi]}{[Fructose-1-P]}

Initial conditions:

[Fructose-1-P]=0.2M

[Fructose]=0M

[Pi]=0M

Equilibrium conditions:

[Fructose-1-P]=6.52*10^{-5}M

[Fructose]=0.2M-6.52*10^{-5}M

[Pi]=0.2M-6.52*10^{-5}M

K_{eq}=\frac{(0.2M-6.52*10^{-5}M)*(0.2M-6.52*10^{-5}M)}{6.52*10^{-5}M}

K_{eq}=613.1

Free-energy for T=298K (standard):

\Delta G^{\circ}=-8.314\frac{J}{mol*K}*298K*ln(613.1)

\Delta G^{\circ}=-15902 J/mol

3 0
3 years ago
Two ligands, a and b, both form complexes with a particular metal ion. when the metal ion complexes with ligand a, the resulting
egoroff_w [7]

Answer:

because

Explanation:

5 0
3 years ago
If a reaction equation is balanced, then _____.
ryzh [129]
A is the answer to this
7 0
3 years ago
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