Which step would help a student find the molecular formula of a compound from the empirical formula?Multiply the ratio of the actual mass of the compound to the empirical formula mass by the subscripts of the empirical formula.

Subtract the ratio of the actual mass of the compound to the empirical formula mass from the subscripts of the empirical formula.

Divide the ratio of the actual mass of the compound to the empirical formula mass by the subscripts of the empirical formula.

Add the ratio of the actual mass of the compound to the empirical formula mass to the subscripts of the empirical formula.

Answers

Answer 1

Answer:

Answer : Option A) Multiply the ratio of the actual mass of the compound to the empirical formula mass by the subscripts of the empirical formula.

Explanation : To find molecular formula for a compound one needs to follow the below steps using the emphirical formula of that compound.

Step 1) Calculate the empirical formula mass of that compound

Step 2) Take the ratio of gram molecular mass by the empirical formula mass that was obtained in step 1.

Step 3) Multiply each of the subscripts within the empirical formula by the number that is calculated in step 2.

By following these easy steps one can find the molecular formula.

Answer 2

Answer:

The step that would help a student finds the molecular formula of a compound from the empirical formula is by ‘Multiply the ratio of the actual mass of the compound to the empirical formula mass by the subscripts of the empirical formula.’

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How many Atoms are in 2.3 g of Na? show your work and these question will take two steps

Answers

Use stoichiometry and convert 2.3 grams of sodium to moles. Then convert the moles to atoms using 6.02(10)^23.

Post your answer and I'll post mine :)

How many grams of KOH used to make 1.6 liters of 15% by mass solution with water as the solvent?

Answers

Given:

KOH used to make 1.6 liters of 15% by mass solution with water

Required:

grams of KOH

solution:

the density of KOH is equal to 2.12 kg/L

multiply the known volume of KOH to the density and the percentage of KOH in water

mass of KOH = 1.6 L (2.12 kg/L)(0.15) = 22.61 grams of KOH

An atom that is electrically neutral containsa. more electrons than protons.
b. more neutrons than electrons.
c. an equal number of neutrons and protons.
d. an equal number of protons and electrons.

Answers

D. I wouldn't bother much with B and C since neutron doesn't necessarily has to be in the picture. So, why D? reasons being, an atom will not be electrically neutral if it exists as an ion. In other words, the no. of electrons have to be the same with the no. of protons.

If 62.8 g Ca react with 92.3 g HCl according to the reaction below, how many grams of hydrogen gas will be produced, and how many grams of the excess reactant will be left over?Unbalanced equation: Ca + HCl → CaCl2 + H2

Answers

Answer:

2.53 grams of hydrogen gas will be produced and 12.2 many grams of the excess reactant i.e. calcium will be left over.

Explanation:

$Ca + 2HCl\rightarrow CaCl_2 + H_2$

Moles of calcium = $(62.8 g)/(40 g/mol)=1.57 mol$

Moles of HCl = $(92.3 g)/(36.5 g/mol)=2.53 mol$

According to reaction, 2 moles of HCl reacts with 1 mole of calcium :

Then 2.53 moles of HCl will recat with :

$(1)/(2)* 2.53 mol= 1.265 mol$ of calcium.

As we can see moles of calcium are in excessive amount. Hence calcium is an excessive reagent.

Moles of calcium left unreacted =1.57 mol - 1.265 mol =0.305 mol

Mass calcium left unreacted = 0.305 mol × 40 g/mol =12.2 g

Since, calcium is an excessive reagent HCl is limiting reagent and the amount of hydrogen gas produced will depend on HCl .

According to reaction, 2 moles of HCl gives 1 mole of hydrogen gas.

Then 2.53 moles of HCl will give:

$(1)/(2)* 2.53 mol= 1.265 mol$ of hydrogen gas.

Mass of 1.265 mol of hydrogen gas = 1.265 mol × 2 g/mol = 2.53 g

2.53 grams of hydrogen gas will be produced and 12.2 many grams of the excess reactant i.e. calcium will be left over.

Answer:

2.55 g of hydrogen

12.17 g calcium.

to nearest hundredth.

Explanation:

The balanced equation is:

Ca + 2HCl ---> CaCl2 + H2

Using the atomic masses

40.078 g Ca react with 72.916 g of HCl to give 2.016 g HCl

The ratio of Ca to HCl in the above is 1 to 1.81935

so 62.8 g Ca reacts with 62.8 * 1.81935 = 114.245 g HCl

so there is excess of Ca in the given weights.

Therefore the mass of Hydrogen produced

= (2.016 / 72.916) * 92.3

= 2.552 g of hydrogen gas.

The mass of calcium required to produce 2.552 g of hydrogen is:

(2.552 / 2.016) * 40.078

= 50.73 g

So the excess of calcium is 62.8 - 50.73

= 12.17 g.

The empirical formula of styrene is CH; find the % composition for H and CH. How many atoms are present in a 2.00 gram sample of styrene? PLEASE HELP! THANK YOU

Answers

% Composition = ?
no atom in 2 g of styrene =?
molar mass of strene =104.15
% composition of c= 12/13.008 =.922*100=92.2
% composition of h =1.008/13.008=0.0774*100= 7.74

no gram atom=mass in kg /molar mass=2/104.15 =0.01920 mol
no of gram atom * avogadro's number = 0.0192*6.02 *10( exponent 23) =1.15584

PLS HELP What is chemistry?

Answers

Answer:

A branch of science

Explanation:

CHemistry is the investigation and studying substances and their reaction with other elements

Answer:

chemistry :-

A branch of science in which we. . study about chemical

in the chemistry we studied about. elements and compounds and their

composition and reaction

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