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ELEN [110]
3 years ago
5

How many grams of CaF2 would be needed to produce 1.23 moles of F2?

Chemistry
1 answer:
NemiM [27]3 years ago
5 0

We see from the chemical formula itself that there is 1 mole of F2 for every 1 mole of CaF2, hence the number of moles of CaF2 is also:

moles CaF2 = 1.23 moles

 

The molar mass of CaF2 is 78.07 g/mol, so the mass is:

mass CaF2 = 78.07 g / mol * 1.23 mol

<span>mass CaF2 = 96.03 grams</span>

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4 0
3 years ago
How many moles of KOH are required to produce 4.79 g K3PO4 according to the following reaction? 3KOH + H3PO4 -----&gt; K3PO4 + 3
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Answer:

0.677 moles

Explanation:

Take the atomic mass of K = 39.1, O =16.0, P = 31.0

no. of moles = mass / molar mass

no. of moles of K3PO4 used = 4.79 / (39.1x3 + 31 + 16x4)

= 0.02256 mol

From the equation, the mole ratio of KOH : K3PO4 = 3 :1,

meaning every 3 moles of KOH used, produces 1 mole of K3PO4.

So, using this ratio, let the no. of moles of KOH required to be y.

\frac{3}{1} =\frac{y}{0.02256} \\

y = 0.02256 x3

y = 0.0677 mol

If you don't find exactly 0.677 moles as one of the options, go for the closest one. A very slight error may occur because of taking different significant figures of atomic masses when calculating.

5 0
3 years ago
Calculate the equilibrium constant K for the following reaction: H2(g) +
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Answer:

192.9

Explanation:

From the question,

Ke = [HCL]²/[H₂][CL₂].......................... Equation 1

Where Ke = Equilibrium constant.

Given: [HCL] = 0.0625 M, [H₂] = 0.0045 M, [CL₂] = 0.0045 M

Substitute these values into equation 1

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ke = 1.929×10²

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2 years ago
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A solution that contains a large amount of salt and a small amount of water is said to be a _______ solution. A. diffused B. uns
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Answer:

D. Concentrated

Explanation:

5 0
3 years ago
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