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3 years ago

Twelve more than sixteen times a number is equal to 2. what is the number?

Chemistry

1 answer:

ASHA 777 [7]3 years ago

6 0

A) -5/8
begin with the equation 12+16n and set it equal to two. Then continue to solve for N or x if you prefer.

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The osmotic pressure of a solution containing 2.04 g of an unknown compound dissolved in 175.0 mLof solution at 25 ∘C is 2.13 at

kherson [118]

Answer: The molecular formula of the compound is $C_4H_{10}O_4$

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

Or,

$\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT$

where,

$\pi$ = osmotic pressure of the solution = 2.13 atm

i = Van't hoff factor = 1 (for non-electrolytes)

Given mass of compound = 2.04 g

Volume of solution = 175.0 mL

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$2.13atm=1\times \frac{2.04\times 1000}{\text{Molar mass of compound}\times 175.0}\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 298K\\\\\text{Molar mass of compound}=\frac{1\times 2.04\times 1000\times 0.0821\times 298}{2.13\times 175.0}=133.9g/mol$

Calculating the molecular formula:

The chemical equation for the combustion of compound 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 $CO_2=36.26g$

Mass of $H_2O=14.85g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

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

So, in 36.26 g of carbon dioxide, $\frac{12}{44}\times 36.26=9.89g$ of carbon will be contained.

For calculating the mass of hydrogen:

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

So, in 14.85 g of water, $\frac{2}{18}\times 14.85=1.65g$ of hydrogen will be contained.

Mass of oxygen in the compound = (22.08) - (9.89 + 1.65) = 10.54 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{9.89g}{12g/mole}=0.824moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1.65g}{1g/mole}=1.65moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{10.54g}{16g/mole}=0.659moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.659 moles.

For Carbon = $\frac{0.824}{0.659}=1.25\approx 1$

For Hydrogen = $\frac{1.65}{0.659}=2.5$

For Oxygen = $\frac{0.659}{0.659}=1$

Converting the mole fraction into whole number by multiplying the mole fraction by '2'

Mole fraction of carbon = (1 × 2) = 2

Mole fraction of oxygen = (2.5 × 2) = 5

Mole fraction of hydrogen = (1 × 2) = 2

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 2 : 5 : 2

The empirical formula for the given compound is $C_2H_5O_2$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

We are given:

Mass of molecular formula = 133.9 g/mol

Mass of empirical formula = 61 g/mol

Putting values in above equation, we get:

$n=\frac{133.9g/mol}{61g/mol}=2$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(2\times 2)}H_{(5\times 2)}O_{(2\times 2)}=C_4H_{10}O_4$

Hence, the molecular formula of the compound is $C_4H_{10}O_4$

4 0

3 years ago

Why do lows appear where there are more clouds and Highs appear where it is clear? (EXPLAIN)

7nadin3 [17]

If you mean temperature wise then it’s due to the clouds absorbing most of the sunlight, less clouds let’s more light through

4 0

2 years ago

Znco3 has a molar mass of 125.40 g/mol. which of the conversion factors shown below correctly expresses this relationship as wel

Airida [17]

Answer : $ZnCO_{3}$ will be 1 mole of $ZnCO_{3}$ / 125. 40 g of $ZnCO_{3}$

Explanation : The molar mass and the formula units are the same thing in any compound so when given a molar mass of compound then one mole of that compound is divided by its molar mass. Where one mole will be equal to avogadro's number which is 6.022 X $10^{23}$ .

4 0

3 years ago

Read 2 more answers

Typically, the hydrogen gas is bubbled through water for col- lection and becomes saturated with water vapor. Suppose 240. mL of

klio [65]

Answer:PH2=0.994atm, mass of zinc=0.606g

Explanation:

Equation for the reaction is written as;

Zn(s) + 2HCl(aq) - ZnCl2(aq) + H2(g)

V= 240ml = 0.240L

T= 30.8oC = 303.8K

Ptotal= 1.036atm

Pwater = 32mmHg at 30oC = 0.042atm

Therefore

PH2 = Ptotal - Pwater

= 1.036-0.042atm

=0.994atm

But PV= nRT

n = PV/RT

= 0.994x0.240/0.0821x303.8

= 0.24/24.94

=0.009324moles

For the grams of zinc

n=mass in grams/molar mass

Mass in grams = no of moles x molar mass

=0.009324x65 = 0.606g

3 0

3 years ago

7 What is the name of this isotope? Periodic Table link P: 36 N: 48

andre [41]

Answer:

Because the number of neutrons is different, the mass number is different. Isotopes are written in two different ways. They can be written using their symbol with the mass number (to the upper left) and atomic number (to the lower left) or the isotope name is written with a dash and the mass number

Explanation:

I don't know the answer but I am sure this will help you out.

6 0

3 years ago