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3 years ago

35.5 moles of lithium fluoride is dissolved in 65 L of solution

Chemistry

1 answer:

kkurt [141]3 years ago

3 0

Answer:

Explanation:

1.10

of solution

Explanation:

The Molarity

is calculated by the equation comparing moles of solute to liters of solution

For this question we are given the Molarity 0.88M

We are told the solute is a 25.2 gram sample of LiF, Lithium Fluoride

We can convert the mass of LiF to moles by dividing by the molar mass of LiF

Li = 6.94

F = 19.0

LiF = 25.94 g/mole

25.2

25.94

0.97

moles

Now we can take the the molarity and the moles and calculate the Liters of solution

0.97

0.88

1.10

of solution i just did look at my papaer

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Ymorist [56]

Answer:

A/1. 10.9 mol O2

Explanation:

583 g x 1 mol SO3 x 3 mol O2 /

80.057 g mol SO3 x 2 mol SO3

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- Everything else came from formula. Further explanation...

- Always start with what they give, such as 583 g. Then find 1 mol of what is being produced, in this it is SO3. We already found this because we did molar mass above. Next. find how many moles of what they want, which is O2. Look in equation and you can see 3 mol in from of O2. Next, do the same for SO3 and you can find 3 mol in front of that. Lastly, just do the math.

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Problem 4

Hunter-Best [27]

<h3>Answer:</h3>

1.93 g

<h3>Explanation:</h3>

<u>We are given;</u>

The chemical equation;

2C₂H₆(g) + 7O₂(g) → 4CO₂(g) + 6H₂O(l) ΔH = -3120 kJ

We are required to calculate the mass of ethane that would produce 100 kJ of heat.

From the equation given;

2 moles of ethane burns to produce 3120 Kilo joules of heat

Therefore;

Number of moles that will produce 100 kJ will be;

= (2 × 100 kJ) ÷ 3120 kJ)

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Therefore;

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Answer:

(See explanation for further details)

Explanation:

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$n = \frac{4.15\times 10^{23}\,molecules}{6.022\times 10^{23}\,\frac{molecules}{mol} }$

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