Question

If there are 4.60 mol of O, how many of each of the following compounds are present?

H2SO4

C2H4O2

NaOH

Answer #1

Given that moles of O = 4.6 mol

1) H2SO4

1 mol of H2SO4 = 2 mol of H + 1 mol of S + 4 mol of O

Hence,

1 mol of H2SO4 = 4 mol of O

So, ? mol of H2SO4 = 4.6 mol of O

? = 1 mol of H2SO4 x (4.6 mol of O / 4 mol of O)

= 1.15 mol of H2SO4

Therefore, 1.15 mol of H2SO4 is present.

2) C2H4O2

1 mol of C2H4O2 = 2 mol of C + 4 mol of H + 2 mol of O

Hence,

1 mol of C2H4O2 = 2 mol of O

So, ? mol of C2H4O2 = 4.6 mol of O

? = 1 mol of C2H4O2 x (4.6 mol of O / 2 mol of O)

= 2.3 mol of C2H4O2

Therefore, 2.3 mol of C2H4O2 is present.

3) NaOH

1 mol of NaOH = 1 mol of Na + 1 mol of O + 1 mol of H

Hence,

1 mol of NaOH = 1 mol of O

So, ? mol of NaOH = 4.6 mol of O

? = 1 mol of NaOH x (4.6 mol of O / 1 mol of O)

= 4.6 mol of NaOH

Therefore, 4.6 mol of NaOH is present.

How many moles of carbon atoms are there in 4 mol of each of the
following compounds?
Calcium carbonate, CaCO3. Express your answer numerically in
moles.
Urea, CO(NH2)2. Express your answer numerically in moles.
Ethylene glycol, C2H6O2. Express your answer numerically in
moles.

How many ammonium ions and how many sulfate ions are present in
an 0.280 mol sample of (NH4)2SO4?
How many atoms of N, H, S, and O are contained in this
sample?

Give the empirical formula of each of the following compounds if
a sample contains the following quantities of each element. (Type
your answer using the format CO2 for CO2.)
(a) 0.0209 mol iron and 0.0313 mol oxygen
(b) 16.8 g C, 1.20 g H, and 6.40 g O
(c) 25.9% nitrogen and 74.1% oxygen by mass

1.How many grams of NaOH required to be dissolved in a
solution containing 0.05M H2SO4 so that the PH of will become
13
(molecular weight for NAOH is 40 g/mol)
2.When we add 0.1 mol from KOH to one liter of
solution of 0.1M H2SO4,the PH of the resulting solution will be
(1,2,4)?

How many moles of O atoms are contained in 2.10 mol of iron(III)
sulfate, Fe2(SO4)3?

4.60 mol of solid A was placed in a sealed 1.00-L container and
allowed to decompose into gaseous B and C. The concentration of B
steadily increased until it reached 1.10 M, where it remained
constant.
A(s)=B(g)+C(g)
Then, the container volume was doubled and equilibrium was
re-established. How many moles of A remain
? mol A

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(scientific Notation)
2.66 mol S8
0.799 mol NH3
10.5 g of C2H5OH
1292 g of Cl2

1.. How many atoms of O in 7.80g of Ca(ClO3)2?
2 How many liters (at STP) are 4.39 x 10 ^25 molecules of
nitrogen monoxide?
3. How many grams of NaOH are in 250.0 ml of a 5.0 M
solution?

For each of the following acid-base reactions, calculate how
many grams of each acid are necessary to completely react with and
neutralize 2.3 g of the base.
A.)
HCl(aq)+NaOH(aq)→H2O(l)+NaCl(aq)
B.)
2HNO3(aq)+Ca(OH)2(aq)→2H2O(l)+Ca(NO3)2(aq)
C.)
H2SO4(aq)+2KOH(aq)→2H2O(l)+K2SO4(aq)
Express your answer using two significant
figures.

In the following reaction, how many grams of sodium sulfate,
Na2SO4, will be produced from 88.3 g of sodium hydroxide, NaOH?
2NaOH + H2SO4 --> Na2SO4 + 2H2O

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