Answer:
The balloon most likely shrank.
Explanation:
<span>Answer: 6.1 g of Ca(NO₃)₂•4H₂O and 5.5 g of KIO₃
</span>
<span>Explanation:
</span>
1) Calculate the number of moles of <span>Ca(NO₃)₂ in 10.0 g
</span>
i) molar mass of <span>Ca(NO₃)₂ = 40.1 g/mol + 2x126.9 g/mol + 2x3x16.0 g/mol = 389.9 g/mol
</span>
<span>ii) Formula: number of moles = mass in grams / molar mass
</span>number of moles = 10.0 g / 389.9 g/mol = 0.02565 moles of Ca(NO₃)₂
<span>
</span><span>2) Write the chemical equation to state the mole ratio:</span>
<span />
<span>i) Ca(NO₃)2•4H₂O(s) + 2KIO₃(s) --> Ca(IO₃)₂(s) + 2KNO₃ + 4H₂O
</span>
ii) mole ratio: 1 mol Ca(NO₃)2•4H₂O(s) : 2 mol KIO₃(s) : 1 mol <span>Ca(IO₃)₂(s)
</span>
3) Use proportionality to find the actual number of moles
<span>
</span><span>i) </span>Ca(NO₃)₂•4H₂O(s)
1 mol <span>Ca(NO₃)₂•4H₂O(s) / 1 mol Ca(IO₃)₂ = x / 0.02565 mol Ca(IO₃)₂ => x = 0.02565 mol </span>Ca(NO₃)₂•4H₂O(s)
molar mass of <span><span>Ca(NO₃)₂•4H₂O(s)</span> = 40.0g/mol + 2x14.0g/mol + 2x3x16.0g/mol + 4x18.0g/mol = 236.0g/mol
</span>
<span>mass in grams = number of moles x molar mass = 0.02565 mol x 236.0 g/mol = 6.1 g
</span>ii) KIO₃
<span />
<span>1mol KIO₃/1molCa(IO₃)₂ = x / 0.02565 mol Ca(IO₃)₂ => x = 0.02565 mol KIO₃</span>
<span>molar mas of KIO₃ = 39.1 g/mol + 126.9 g/mol + 3x16.0 g/mol = 214.0 g/mol
</span>
mass in grams = 0.02565 mol x 214.0 g/mol = 5.5 g
Pure water does
not have enough ions to conduct electricity. A mixture of metals such as iron,
zinc and copper in the wet soil can trigger electrolysis that requires excess
energy in the form of over potential to conduct electricity. The excess energy
is needed due to limited self-ionization of water. The wet soil then can
conduct current when positive and negative ions are present. The water ions begin
to flow from anode (positive electrode) to cathode (negative electrode) to be oxidize
and produce electricity.
<span> </span>
The limiting reactant is Cl₂ (chlorine).
Explanation:
We have the following chemical reaction:
2 Al (s) + 3 Cl₂ (g) → 2 AlCl₃ (s)
And we start with 2.7 g of Al and 3.12 g of Cl₂.
First we calculate the number of moles of each reactant.
number of moles = mass / molar weight
number of moles of Al = 2.7 / 27 = 0.1 moles
number of moles of Cl₂ = 3.12 / 71 = 0.044 moles
From the chemical reaction we see that 2 moles of Al are reacting with 3 moles of Cl₂ so 0.1 moles of Al are reacting with 0.15 moles of Cl₂ which is a quantity higher than our available one of 0.044 moles of Cl₂. The limiting reactant is Cl₂.
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limiting reactant
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