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3 years ago

SHOW ALL WORK AND INCLUDE UNITS

Chemistry

1 answer:

Sliva [168]3 years ago

6 0

Answer:

+375.2 KJ.

Explanation:

The balanced equation for the reaction is given below:

H₂ + F₂ —> 2HF ΔH = +536 KJ

From the balanced equation above,

2 moles of HF required +536 KJ .

Finally, we shall determine the heat required to produce 1.4 mol of hydrogen fluoride, HF. This is illustrated below:

From the balanced equation above,

2 moles of HF required +536 KJ .

Therefore, 1.4 moles of HF will require = (1.4 × 536)/2 = +375.2 KJ

Thus, +375.2 KJ of heat energy is required.

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What are the properties of organic compounds determined by?

jarptica [38.1K]

The properties of organic compounds is determined by <u>A) Their boiling point</u><u />.

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3 years ago

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If 5.12 liters of a 2.75 M phosphoric acid is neutralized by magnesium hydroxide solution of 4.00 M.

Tresset [83]

Answer:

5.28 L

Explanation:

Step 1:

Data obtained from the question.

Volume of acid (Va) = 5.12L

Molarity of acid (Ma) = 2.75M

Molarity of base (Mb) = 4M

Volume of base (Vb) =.?

Step 2:

The balanced equation for the reaction

2H3PO4 + 3Mg(OH)2 → Mg3(PO4)2 + 6H2O

From the balanced equation above,

Mole ratio of the acid (nA) = 2

Mole ratio of the base (nB) = 3

Step 3:

Determination of the volume of the base.

This is illustrated below:

MaVa/MbVb = nA/nB

2.75 x 5.12 / 4 x Vb = 2/3

Cross multiply

4 x 2 x Vb = 2.75 x 5.12 x 3

Divide both side by 4 x 2

Vb = (2.75 x 5.12 x 3)/(4 x 2)

Vb = 5.28 L

Therefore, the volume of the base is 5.28 L

8 0

3 years ago

Read 2 more answers

Cal is titrating 50.8 mL of 0.319 M HBr with 0.337 M Ba(OH)2. How many mL of Ba(OH)2 does Cal need to add to reach the equivalen

alexgriva [62]

Answer:

$V_{base}=24.04mL$

Explanation:

Hello!

In this case, according to the chemical reaction by which HBr reacts with Ba(OH)2:

$2HBr+Ba(OH)_2\rightarrow BaBr_2+2H_2O$

We can see there is a 2:1 mole ratio between the acid and the base; thus, at the equivalent point we can write:

$2M_{base}V_{base}=M_{acid}V_{acid}$

Therefore, for is to compute the volume of the used base, we proceed as shown below:

$V_{base}=\frac{M_{acid}V_{acid}}{2M_{base}}$

And we plug in to obtain:

$V_{base}=\frac{0.319M*50.8mL}{2*0.337M}\\\\V_{base}=24.04mL$

Best regards!

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3 years ago

What would you predict about a chemical that has a hydrogen ion concentration of 1×10 to the -12

KonstantinChe [14]

Answer:

It is basic.

Explanation:-

Given hydrogen ion concentration [H+] = 1×10^-12

Using the formula

pH = - log [H+]

= - log [ 1 x 10^-12]

= 12

Since the pH is more than 7, the chemical is basic

3 0

3 years ago

Determine whether a precipitate will form when 0.96g of Na2CO3 is combined with 0.20g BaBr2 in a 10 L solution.

Mashcka [7]

Answer:

Qsp > Ksp, BaCO3 will precipitate

Explanation:

The equation of the reaction is;

Na2CO3 + BaBr2 -------> 2NaBr + BaCO3

Since BaCO3 may form a precipitate we can determine the Qsp of the system.

Number of moles of Na2CO3 = 0.96g/106 g/mol = 9.1 * 10^-3 moles

concentration of NaCO3 = number of moles/volume of solution = 9.1 * 10^-3 moles/10 L = 9.1 * 10^-4 M

Number of moles of BaBr2 = 0.20g/297 g/mol = 6.7 * 10^-4 moles

concentration of BaBr2 = 6.7 * 10^-4 moles/10 L = 6.7 * 10^-5 M

Hence;

[Ba^2+] = 6.7 * 10^-5 M

[CO3^2-] = 9.1 * 10^-4 M

Qsp = [6.7 * 10^-5] [9.1 * 10^-4]

Qsp = 6.1 * 10^-8

But, Ksp for BaCO3 is 5.1*10^-9.

Since Qsp > Ksp, BaCO3 will precipitate

3 0

3 years ago