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3 years ago

ASAP PLEASE I NEED TO BALANCE THEM PLZ HELP IM FAILING THANKS ILL GIVE BRAINLIEST

Chemistry

1 answer:

a_sh-v [17]3 years ago

7 0

Answer:

4H₂O(l) → 4H₂(g) + 2O₂(g)

Balancing equations

1. 3Fe(s) + 4H₂O(g) → Fe₃0₄(s) + 4H₂(g)

2. 2AlBr₃(aq) + 3Cl₂(g) → 2AlCl₃(aq) + 3Br₂(l)

3. 2HNO₃(aq) + Ba(OH)₂(aq) → Ba(NO₃)₂(aq) + 2H₂O(l)

4. 2Al(s) + 3Pb(NO₃)₂ → 2Al(NO₃)₃(aq) + 3Pb(s)

5. 3NaOH(aq) + Fe(NO₃)₃ → Fe(OH)₃(s) + 3NaNO₃(aq)

Explanation:

From the question given, I have been able to balance the chemical equations correctly.

In balancing chemical equations, the chemical equation must have equal number of atoms for each element that are both in the reactant side and in the product side.

For the above to be achieved, the number of atoms in each element will have to be multiplied and added.

A look at the balanced chemical equation above, you will discover that each element has the same number of atoms both in the reactant side and in the product side.

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Calculate the percent water in iron ii sulfate heptahydrate

liq [111]

According to its formula FeSO4.7H2O
we can get the percent % by the mass of H2O from this formula
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when the mass of water = molar mass x 7 = 18 x 7 = 126
and the mass of hydrate (feSO4) = molar mass = 278
So by substitution:
%mass of H2O = (126/278) x 100 = 45%

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3 years ago

Metals show a wide range of chemical behavior. Give examples of that variation by describing some common properties of calcium,

Alex17521 [72]

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4 years ago

Read 2 more answers

Use tabulated standard electrode potentials to calculate the standard cell potential for the following reaction occurring in an

SVETLANKA909090 [29]

Answer : The standard cell potential of the reaction is, -1.46 V

Explanation :

The given balanced cell reaction is,

$3Pb^{2+}(aq)+2Cr(s)\rightarrow 2Cr^{3+}(aq)+3Pb(s)$

Here, chromium (Cr) undergoes oxidation by loss of electrons and act as an anode. Lead (Pb) undergoes reduction by gain of electrons and thus act as cathode.

The standard values of cell potentials are:

Standard reduction potential of lead $E^0_{[Pb^{2+}/Pb]}=-0.13V$

Standard reduction potential of chromium $E^0_{[Cr^{3+}/Cr]}=1.33V$

Now we have to calculate the standard cell potential for the following reaction.

$E^0=E^0_{cathode}-E^0_{anode}$

$E^0=E^0_{[Pb^{2+}/Pb]}-E^0_{[Cr^{3+}/Cr]}$

$E^0=(-0.13V)-1.33V=-1.46V$

Therefore, the standard cell potential of the reaction is, -1.46 V

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4 years ago

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Answer:

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3 years ago

A lab technician mixed a 550 ml solution of water and alcohol. if 3% of the solution is alcohol, how many milliliters of alcoh

kupik [55]

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4 years ago