D snails, guppies and plants. The community should be diverse and have lots of biodiversity.
The equilibrium expression shows the ratio between
products and reactants. This expression is equal to the concentration of the
products raised to its coefficient divided by the concentration of the
reactants raised to its coefficient. The correct equilibrium expression for the
given reaction is:<span>
<span>H2CO3(aq) + H2O(l) = H3O+(aq) + HCO3-1(aq)
Kc = [HCO3-1] [H3O+] / [H2O] [H2CO3]</span></span>
Answer:
1461.7 g of AgI
Explanation:
We'll begin by writing the balanced equation for the reaction. This is given below:
CaI₂ + 2AgNO₃ —> 2AgI + Ca(NO₃)₂
From the balanced equation above,
1 mole of CaI₂ reacted to produce 2 moles of AgI.
Next, we shall determine the number of mole AgI produced by the reaction of 3.11 moles of CaI₂. This can be obtained as follow:
From the balanced equation above,
1 mole of CaI₂ reacted to produce 2 moles of AgI.
Therefore, 3.11 moles of CaI₂ will react to produce = 3.11 × 2 = 6.22 moles of AgI
Finally, we shall determine the mass of 6.22 moles of AgI. This can be obtained as follow:
Mole of AgI = 6.22 moles
Molar mass of AgI = 108 + 127
= 235 g/mol
Mass of AgI =?
Mass = mole × molar mass
Mass of AgI = 6.22 × 235
Mass of AgI = 1461.7 g
Therefore, 1461.7 g of AgI were obtained from the reaction.
yield = 52.23 %
Explanation:
We have the following chemical reaction:
2 Al (s) + 2 KOH (aq) + 4 H₂SO₄ (aq) + 10 H₂O → 2 KAl(SO₄)₂·12 (H₂O) (s) + 3 H₂ (g)
mass of aluminium = mass of bottle with aluminium pieces - bottle mass
mass of aluminium = 10.8955 - 9.8981 = 0.9974 g
mass of alum = mass of bottle with final product - bottle mass
mass of alum = 19.0414 - 9.8981 = 9.1433 g
number of moles = mass / molecular weight
number of moles of aluminium = 0.9974 / 27 = 0.03694 moles
number of moles of alum (practical) = 9.1433 / 474 = 0.01929 moles
To calculate the theoretical quantity of alum that should be obtained from 0.03694 moles of aluminium we devise the following reasoning:
if 2 moles of aluminium produce 2 moles of alum
then 0.03694 moles of aluminium produce X moles of alum
X = (0.03694 × 2) / 2 = 0.03694 moles of alum (theoretical)
yield = (practical quantity / theoretical quantity) × 100
yield = (0.01929 / 0.03694) × 100
yield = 52.23 %
Learn more about:
reaction yield
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A polymer is a really long chain of smaller molecules (monomers). It's similar to a chain of paper clips because all of the little monomers will attach to each other, forming a long strain.
