A group of students investigated the chemical

Calculate the percent mass of sugar in mountain dew: The total mass of the mountain dew solution is 300g and there are 231 g of

s2008m [1.1K]

Answer:

c. 77 %

Explanation:

Percent mass (% mass) of solute = mass of solute/mass of solution × 100

According to this question, a mountain dew solution weighing 300grams contains 231 g of sugar. This means that:

% mass of sugar = 231g/300g × 100

% mass of sugar = 0.77 × 100

% mass of sugar = 77%.

4 0

2 years ago

Draw the isotopic notation for an element with 15 protons, 18 neutrons and 18 electrons

tatiyna

Answer:

can't be done

Explanation:

protons and electrons always are the same number,and the neutrons are found by subtracting the atomic mass and protons/electrons soooooooo it can't have 15 protons, 18 electrons, and 18 neutrons.......i hope this helped if not please tell me.

5 0

2 years ago

If 15 grams of Carbon dioxide is produced in a chemical reaction, how many grams of Carbon must be consumed in the reaction if w

Nata [24]

4.1g

Explanation:

Given parameters:

Mass of carbon dioxide = 15g

Mass of oxygen gas = 11g

Unknown:

Mass of carbon consumed = ?

Solution:

Equation of the reaction:

C + O₂ → CO₂

To solve this problem from the balanced equation, we have to use the amount of product formed and work to Carbon. This is because, we are sure of the amount of carbon dioxide formed but the amount of the given oxygen gas used is not precise.

Number of moles of CO₂ = $\frac{mass}{molar mass}$

Molar mass of CO₂ = 12 + (16 x2) = 44g/mol

Number of moles of CO₂ = $\frac{15}{44}$ = 0.34mole

From the equation of the reaction;

1 mole of CO₂ is produced from 1 mole of C

0.34mole of CO₂ will produce 0.34mole of C

Mass of carbon reacting = number of moles x molar mass = 0.34 x 12 = 4.1g

Learn more:

Number of moles brainly.com/question/1841136

#learnwithBrainly

4 0

2 years ago

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 these describes a Mole in Chemistry?

olya-2409 [2.1K]

Answer: Thus the correct option is D. All of the above describe a mole

Explanation:

According to avogadro's law, 1 mole of every substance weighs equal to molecular mass in grams.

1 mole of every substance contains avogadro's number $6.023\times 10^{23}$ of particles.

Mole is the S.I unit for measuring the amount of substance. It is often used to measure large number of particles.

Thus the correct option is D. All of the above describe a mole

5 0

2 years ago