29 ) Consider the reaction: ___H 2 O 2(aq) ___H 2 O (l) + ___O 2(g) Balance the

Question

29 )

Consider the reaction: ___H2O2(aq) ___H2O(l)  + ___O2(g)

Balance the chemical equation.

Enter coefficient values from left to right separated by commas. For example: 1,2,3

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If all of the O2 gas that is produced when 5.00 g of H2O2 decomposes is captured in a 1.25 L container, what will be the pressure at 298K?

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Determine the empirical formula of a compound that is 64.80% M, 13.62% X, and 21.58% E by mass.

molar mass of M = 18.015 g/mole

molar mass of X = 1.512 g/mole

molar mass of E = 23.999 g/mole

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Q 27 )

60.54 g of an ideal gas occupies 67.2 L at STP. What is the molar mass of the gas?

Part B

Determie the identity of the gas.

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Q 26 )

What are the correct coefficients (reading from left to right) when the chemical equation is balanced?

____ M2X3 + ____ E    ____ M + ____ EX2

Write answer as numbers separted by commas. For example: 1,2,3

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Q 25 )

Which is an example of an oxidation-reduction reaction?

Which is an example of an oxidation-reduction reaction?

AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

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Item 24

Consider the balanced redox reaction:

Cu(s) + ZnSO4(aq) CuSO4(aq) + Zn(s)

Copper has an initial oxidation state of ______ and a final oxidation state of _______.

Enter values separated by commas. For example: 1+,2+

B)

Zinc has an initial oxidation state of ______ and a final oxidation state of _______.

Enter values separated by commas. For example: 1+,2+

C)

Sulfate has an initial oxidation state of ______ and a final oxidation state of _______.

Enter values separated by commas. For example: 1+,2+

4Fe(s) + 3O2(g) 2Fe2O3(s) CaCO3(s) CaO(s) + CO2(g) 2AlCl3(aq) + 3Na2O(aq) Al2O3(s) + 6NaCl(aq)

AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

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Item 24

Consider the balanced redox reaction:

Cu(s) + ZnSO4(aq) CuSO4(aq) + Zn(s)

Copper has an initial oxidation state of ______ and a final oxidation state of _______.

Enter values separated by commas. For example: 1+,2+

B)

Zinc has an initial oxidation state of ______ and a final oxidation state of _______.

Enter values separated by commas. For example: 1+,2+

C)

Sulfate has an initial oxidation state of ______ and a final oxidation state of _______.

Enter values separated by commas. For example: 1+,2+

Explanation / Answer

29 )

Consider the reaction: _2__H2O2(aq) _2__H2O(l)  + __1_O2(g)

   2,2,1

30. 2H2O2 -------> 2H2O + O2

     2 moles of H2O2 decomposes to gives 1 mole of O2

    2*34g of H2O2 decomposes to gives 32g of O2

    5g of H2O2 decomposes to gives = 32*5/2*34 = 2.35g of O2

PV = nRT

n = W/M = 2.35/32 = 0.0734 moles

V = 1.25L

T = 298K

R = 0.0821L-atm/mole-k

P = nRT/V

= 0.0734*0.0821*298/1.25 = 1.44atm

Element     %        A.Wt        Relative number                simple ratio

M            64.8      18.015      64.8/18.015 = 3.59           3.59/0.899 = 4

X            13.62     1.512        13.62/1.512 = 9               9/0.899     = 10

E            21.58     23.999      21.58/23.999 = 0.899    0.899/0.899   = 1

Empirical formula is M4X10O

27. PV = nRT

    n    = W/M

   P = 1 at STP

   T = 273 at STp

PV   = WRT/M

M   = WRT/PV

     = 60.54*0.0821*273/1*67.2   = 20.2 g/mole (Ne)

26. ___2_ M2X3 + __3__ E    __4__ M + ___3_ EX2

       2,3,4,3

25. 4Fe(s) + 3O2(g) 2Fe2O3(s)

24.

Cu(s)0 + ZnSO4(aq) Cu2SO42-(aq) + Zn(s)

Cu0 + Zn+2 -------> Cu+2 + Zn0

copper oidation number   0 to +2

Zinc oxidation number +2 to 0

sulpur oxidation number no change +6 to +6

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