How many moles of solute are in 5 liters of a 5 M solution?

The molar heat of fusion of gold is 12.550 kJ mol–1. At its melting point, how much mass of melted gold must solidify to release

KATRIN_1 [288]

The mass of melted gold to release the energy would be 3, 688. 8 Kg

<h3>How to determine the mass</h3>

The formula for quantity of energy is given thus;

Q = n × HF

Where n represents number of moles

HF represents heat of fusion

To find the number of moles, we have

235.0 = n × 12.550

number of moles = $\frac{235}{12. 550}$ = 18. 725 moles

Note that molar mass of Gold is 197g/ mol

Let's note that;

Number of moles = mass/ molar mass

Mass = number of moles × molar mass

Mass = 18. 725 × 197

Mass = 3, 688. 8 Kg

Thus, the mass of melted gold to release the energy would be 3, 688. 8 Kg

Learn more about molar heat of fusion here:

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8 0

1 year ago

In a certain variety of plants, red flowers appear in majority of plants and blue flowers appear only in a few plants. Which sta

Jlenok [28]

Answer:

C

Explanation:

3 0

3 years ago

Other than reducing greenhouse gas emissions, why would an entity switch to an alternative energy solution

Alika [10]

Answer:

renewable energy sources such as solar and wind DONT emit carbon dioxide and other greenhouse gases that contribute to global warming

Explanation:

8 0

1 year ago

What is the theoretical yield of fluorenone if you oxidize 175 mg of fluorene?

My name is Ann [436]

Answer:

602 mg of CO₂ and 94.8 mg of H₂O

Explanation:

The yield is measured by the amount of each product produced by the reaction.

The chemical formula of fluorene is C₁₃H₁₀, and its molar mass is 166.223 g/mol.

The oxidation, also know as combustion, of this hydrocarbon is represented by the following balanced chemical equation:

$2C_{13}H_{10}+31O_2\rightarrow 26CO_2+10H_2O$

To calculate the yield follow these steps:

1. Mole ratio

$2molC_{13}H_{10}:31molO_2:26molCO_2:10molH_2O$

2. Convert 175mg of fluorene to number of moles

$175mg/times 1g/1,000mg=0.175g$

Number of moles = mass in grams / molar mass

$\text{number of moles}=0.175g/166.223g/mol=0.0010528mol$

3. Set a proportion for each product of the reaction

a) For CO₂

i) number of moles

$2molC_{10}H_{13}/26molCO_2=0.0010528molC_{10}H{13}/x$

$x=0.0010528molC_{10}H_{13}\times 26molCO_2/2molC_{10}H_{13}=0.013686molCO_2$

ii) mass in grams

The molar mass of CO₂ is 44.01g/mol

mass = number of moles × molar mass

mass = 0.013686 moles × 44.01 g/mol = 0.602 g = 602mg

b) For H₂O

i) number of moles

$0.0010528molC_{10}H_{13}\times10molH_2O/2molC_{10}H_{13}=0.00526molH_2O$

ii) mass in grams

The molar mass of H₂O is 18.015g/mol

mass = number of moles × molar mass

mass = 0.00526 moles × 18.015 g/mol = 0.0948mg = 94.8 mg

4 0

3 years ago

How much heat is released when 1.4 mol of hydrogen fluoride are produced? H2(g) +F2(g) → 2HF(g) +536kJ (Please show work)

polet [3.4K]

Answer:

375.2 kJ

Explanation:

H₂(g) +F₂(g) → 2HF(g) +536kJ

The information the equation above provides lets us know that when 2 mol of hydrogen fluoride (HF) are produced, 536 kJ of energy (as heat) is produced.

We can then state a rule of three:

2 mol HF -------- 536 kJ

1.4 mol HF --------- X

And solve for X:

X = 1.4 mol * 536 kJ / 2 mol

X = 375.2 kJ

7 0

2 years ago