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3 years ago

According to the hypothesis the solar system formed from a cloud of dust and gas

Chemistry

2 answers:

pentagon [3]3 years ago

6 0

It not asking it’s actually saying blank etc

katrin2010 [14]3 years ago

5 0

I assume this is a true or false question. I would say true

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Methyl salicylate is a common active ingredient in liniments such as ben-gay. It is also known as oil of wintergreen. It is made

arlik [135]

Answer: The empirical formula is $C_3H_3O$ .

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2$ = 12.24 g

Mass of $H_2O$ = 2.505 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 12.24 g of carbon dioxide, = $\frac{12}{44}\times 12.24=3.338g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 2.505 g of water, = $\frac{2}{18}\times 2.505=0.278g$ of hydrogen will be contained.

Mass of oxygen in the compound = (5.287) - (3.338+0.278) = 1.671 g

Step 1 : convert given masses into moles.

Moles of C = $\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{3.338g}{12g/mole}=0.278moles$

Moles of H= $\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.278g}{1g/mole}=0.278moles$

Moles of O= $\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{1.671g}{16g/mole}=0.104moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{0.278}{0.104}=3$

For H = $\frac{0.278}{0.104}=3$

For O = $\frac{0.104}{0.104}=1$

The ratio of C : H : O = 3: 3: 1

Hence the empirical formula is $C_3H_3O$ .

5 0

3 years ago

Which of the following is not true for atoms?

mariarad [96]

They are able to be divided by a chemical reaction

8 0

4 years ago

What is the mass of 1.45 moles of silver sulfate?

tatuchka [14]

Answer:

449.5 g

Explanation:

Silver sulfate- Ag2SO4

M(Ag)=107 g/mol => M(Ag2)=214 g/mol

M(S)=32 g/mol

M(O)=16 g/mol => M(O4)=64 g/mol

M(Ag2SO4)=310 g/mol

n=1.45 mol

m(Ag2SO4)=M(Ag2SO4)*n=310 g/mol *1.45 mol= 449.5 g

3 0

3 years ago

Read 2 more answers

A person aims for a target with a wooden bow and arrow. The image shows the path of the

Norma-Jean [14]

Answer:

What’s the answer

Explanation:

I neeeddsdd

5 0

3 years ago

which quantity will always have a negative value? A) the total bond energy of the reactants in an endothermic reaction. B) the c

lara [203]

Considering the definition of enthalpy of a chemical reaction and endothermic and exothermic reaction, the correct answer is option C: the change in energy in a system during an exothermic reaction.

The enthalpy of a chemical reaction as the heat absorbed or released in a chemical reaction when it occurs at constant pressure. That is, the heat of reaction is the energy that is released or absorbed when chemicals are transformed into a chemical reaction.

On the other side, an endothermic reaction requires energy while an exothermic reaction releases energy.

In other words, a chemical reaction is endothermic when it absorbs energy from the environment. In this case, the heat is transferred from the outside to the inside of the system.

On the other hand, an exothermic reaction is one where energy flows out of the system. This energy is released in the form of heat.

So, if the enthalpy of reaction is negative, it means that during the course of the reaction, the system loses or releases heat to the environment and is exothermic, while if the enthalpy of reaction is positive, it means that during the course of the reaction, the system absorbs heat from the environment and is endothermic.

So, the correct answer is option C: the change in energy in a system during an exothermic reaction.

Learn more about enthalpy of a chemical reaction and endothermic and exothermic reaction:

6 0

2 years ago