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3 years ago

How many moles of carbon atoms are present in 5.4 moles of glucose? Answer in units of mol.

Chemistry

1 answer:

Delvig [45]3 years ago

3 0

Answer:

32.4 mol

Explanation:

Given data:

Number of moles of C atom present = ?

Number of moles of glucose = 5.4 mol

Solution:

Glucose formula = C₆H₁₂O₆

There are 6 moles of C atoms are present in one mole of glucose.

In 5.4 moles of glucose:

5.4 mol × 6 = 32.4 mol

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Which property of the water molecule causes two water molecules to be attracted to each other?

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Atoms of oxygen are electronegative and attract the shared electrons in their covalent bonds.

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What are the 4 different types of chemical reactions? And how to remember them

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<span>Synthesis, decomposition, single replacement and double replacement.</span>

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How many molecules in 9.18 moles of C11H12O22

Setler [38]

Answer:

55.3 × 10²³ molecules

Explanation:

Given data:

Number of moles of C₁₁H₁₂O₂₂ = 9.18 mol

Number of molecules = ?

Solution:

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

For example,

18 g of water = 1 mole = 6.022 × 10²³ molecules of water

For given data:

9.18 mol × 6.022 × 10²³ molecules /1 mol

55.3 × 10²³ molecules

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3 years ago

Assuming that gasoline is 100% isooctane, that isooctane burns to produce only CO2CO2 and H2OH2O, and that the density of isooct

Aleksandr [31]

Answer:

1.12×10¹¹ kg of CO₂ are produced with 4.6×10¹⁰ L of isooctane

Explanation:

Let's state the combustion reaction:

C₈H₁₈ + 25/2O₂ → 8CO₂ + 9H₂O

Let's calculate the mass of isooctane that reacts.

Density = Mass / Volume

Density . Volume = Mass

First of all, let's convert the volume in L to mL, so we can use density.

4.6×10¹⁰ L . 1000 mL / 1L = 4.6×10¹³ mL

0.792 g/mL . 4.6×10¹³ mL = 3.64 ×10¹³ g

This mass of isooctane reacts to produce CO₂ and water, so let's determine the moles of reaction

3.64 ×10¹³ g . 1mol / 114 g = 3.19×10¹¹ mol

Ratio is 1:8 so 1 mol of isooctane can produce 8 moles of dioxide

Therefore 3.19×10¹¹ mol would produce (3.19×10¹¹ mol . 8) = 2.55×10¹² moles of CO₂

Now, we can determine the mass of produced CO₂ by multipling:

moles . molar mass

2.55×10¹² mol . 44 g/mol = 1.12×10¹⁴ g of CO₂

If we convert to kg 1.12×10¹⁴ g / 1000 = 1.12×10¹¹ kg

6 0

3 years ago

What is the final temperature of a 34.2 g of water initially at 282 K that has been heated with 2.71 kJ of energy?

lana66690 [7]

Answer: The final temperature of copper is

Further explanation:

The property is a unique feature of the substance that differentiates it from the other substances. It is classified into two types:

1. Intensive properties:

These are the properties that depend on the nature of the substance. These don't depend on the size of the system. Their values remain unaltered even if the system is further divided into a number of subsystems. Temperature, refractive index, concentration, pressure, and density are some of the examples of intensive properties.

2. Extensive properties:

These are the properties that depend on the amount of the substance. These are additive in nature when a single system is divided into many subsystems. Mass, enthalpy, volume, energy, size, weight, and length are some of the examples of extensive properties.

Specific heat is the amount of heat required to increase the temperature of any substance per unit mass. Specific heat capacity is also known as mass specific heat. Its SI unit is Joule (J).

The formula to calculate the heat energy of copper is as follows:

…… (1)

Here,

Q is the amount of heat transferred.

m is the mass of copper.

c is the specific heat of copper.

is the change in temperature of copper.

Rearrange equation (1) to calculate the temperature change.

…… (2)

The value of Q needs to be converted into J. The conversion factor for this is,

So the value of Q can b calculated as follows:

The value of Q is 4689 J.

The value of m is 34.2 g.

The value of c is .

Substitute these values in equation (2).

The temperature change can be calculated as follows:

…… (3)

Here,

is the change in temperature.

is the final temperature.

is the initial temperature.

Rearrange equation (3) to calculate the final temperature.

…… (4)

The value of is .

The value of is

Substitute these values in equation (4).

So the final temperature of copper is .

7 0

3 years ago