need help answering questions



What is the empirical formula of a compound composed of 25.1 g

of potassium (K

) and 5.14 g

of oxygen (O

)? Insert subscripts as needed.

empirical formula:



A 17.02

g sample of a compound contains 5.43

g of potassium, K,


g of chlorine, Cl,

and oxygen, O.

Calculate the empirical formula.

Insert subscripts as needed.

Empirical formula:



A 9.32

g sample of a compound contains 5.95

g of iron, Fe,


g of phosphorus, P,

and oxygen, O.

Calculate the empirical formula for the compound.

empirical formula:


Determine the empirical formula for a compound that contains 58.8%

C, 9.8%

H, and 31.4%

S by mass.

empirical formula:


Determine the empirical formula for a compound that is 62.1%

C, 10.4%

H, and 27.5%

O by mass.

empirical formula:


What is the empirical formula of a compound composed of 3.25% hydrogen (H

), 19.36% carbon (C

), and 77.39% oxygen (O

)by mass?

Insert subscripts as needed.

empirical formula:


hw 8

For the chemical reaction shown,


determine how many grams of N2 are produced from the reaction of 9.97

g of H2O2 and 6.35

g of N2H4.


When heated, KClO3

decomposes into KCl

and O2.


If this reaction produced 89.1 g KCl,

how many grams of O2

were produced?

g O2


When 0.540

g of sodium metal is added to an excess of hydrochloric acid, 5610

J of heat are produced. What is the enthalpy of the reaction as written?


When methanol, CH3OH,

is burned in the presence of oxygen gas, O2,

a large amount of heat energy is released, as shown in the combustion reaction.

CH3OH(g)+32O2(g)CO2(g)+2H2O(l)Δ =764 kJ

Based on the balanced thermochemical reaction, how much heat is produced when 33.6 g

of methanol reacts with 52.1 g

of oxygen?

When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced.


How many grams of calcium chloride will be produced when 30.0 g

of calcium carbonate is combined with 12.0 g

of hydrochloric acid?



Which reactant is in excess?

How many grams of the excess reactant will remain after the reaction is complete?

Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia.


Assume 0.200 mol N2

and 0.633 mol H2

are present initially.

After complete reaction, how many moles of ammonia are produced?



How many moles of H2



How many moles of N2



What is the limiting reactant?

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