Answer:
a. HCl.
b. 0.057 g.
c. 1.69 g.
d. 77 %.
Explanation:
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In this case, since the reaction between magnesium and hydrochloric acid is:
Whereas there is 1:2 mole ratio between them.
a) Here, we can identify the limiting reactant as that yielded the fewest moles of hydrogen gas product via the 1:1 and 2:1 mole ratios:
Thus, since hydrochloric yields fewer moles of hydrogen than magnesium, we realize it is the limiting reactant.
b) Here, we use the molar mass of gaseous hydrogen (2.02 g/mol) to compute the mass:
c) Here, we compute the mass of magnesium associated with the yielded 0.0248 moles of hydrogen:
Thus, the mass of excess magnesium turns out:
d) Finally, we compute the percent yield, considering 0.044 g is the actual yield and 0.057 g the theoretical yield:
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F- Fluorine only forms a single bond.
Fluorine has five electrons in its p-orbital. By gaining one electron from the single bond,. Fluorine would then be a stable stony with 8 valence electrons.
Explanation:
Once blood glucose levels increase, pancreatic insulin migrates into a fat cell via the blood stream. Insulin then binds in the plasma membrane of the cell to an Insulin Receptor (IR). Through autophosphorylation, phosphate groups are then added to the IR, causing GLUT4 molecules to come to the cell's surface.
<span>Oxygen, nitrogen, and fluorine bond with hydrogen to form molecules. These molecules are attracted to each other by...
hydrogen bonds. Hydrogen bonding is one of the strongest types of bonding in chemistry. A bond between hydrogen and oxygen, or hydrogen and nitrogen, or hydrogen and fluorine is required for molecules to have hydrogen bonds.</span>
<u>Answer:</u> The equilibrium constant for this reaction is
<u>Explanation:</u>
The equation used to calculate standard Gibbs free change is of a reaction is:
For the given chemical reaction:
The equation for the standard Gibbs free change of the above reaction is:
We are given:
Putting values in above equation, we get:
To calculate the equilibrium constant (at 25°C) for given value of Gibbs free energy, we use the relation:
where,
= standard Gibbs free energy = -32.9 kJ/mol = -35900 J/mol (Conversion factor: 1 kJ = 1000 J )
R = Gas constant = 8.314 J/K mol
T = temperature =
= equilibrium constant at 25°C = ?
Putting values in above equation, we get:
Hence, the equilibrium constant for this reaction is