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mel-nik [20]
3 years ago
6

Hydrazine, N2H4 , reacts with dinitrogen tetroxide, N204.

Chemistry
1 answer:
Virty [35]3 years ago
3 0

Answer:

C

Explanation: thats what i got

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How much energy must be removed from a 125 g sample of benzene (molar mass= 78.11 g/mol) at 425.0 K to liquify the sample and lo
riadik2000 [5.3K]

Answer : The energy removed must be, -67.7 kJ

Solution :

The process involved in this problem are :

(1):C_6H_6(g)(425.0K)\rightarrow C_6H_6(g)(353.0K)\\\\(2):C_6H_6(g)(353.0K)\rightarrow C_6H_6(l)(353.0K)\\\\(3):C_6H_6(l)(353.0K)\rightarrow C_6H_6(l)(335.0K)

The expression used will be:

\Delta H=[m\times c_{p,g}\times (T_{final}-T_{initial})]+m\times \Delta H_{vap}+[m\times c_{p,l}\times (T_{final}-T_{initial})]

where,

\Delta H = heat released by the reaction = ?

m = mass of benzene = 125 g

c_{p,g} = specific heat of gaseous benzene = 1.06J/g^oC

c_{p,l} = specific heat of liquid benzene = 1.73J/g^oC

\Delta H_{vap} = enthalpy change for vaporization = 33.9kJ/mole=33900J/mole=\frac{33900J/mole}{78.11g/mole}J/g=434.0J/g

Molar mass of benzene = 78.11 g/mole

Now put all the given values in the above expression, we get:

\Delta H=[125g\times 1.06J/g.K\times (353.0-(425.0))K]+125g\times -434.0J/g+[125g\times 1.73J/g.K\times (335.0-353.0)K]

\Delta H=-67682.5J=-67.7kJ

Therefore, the energy removed must be, -67.7 kJ

4 0
3 years ago
How do you find the molar mass for ba(NO3)2
Korvikt [17]
To find the molar mass<span> of </span>Ba(NO3)2<span>, determine the </span>molar masses of all the atoms that form it. The Molar mass for Barium nitrate is <span>261.337 g/mol.</span>
8 0
3 years ago
What happens to the individual molecules of a liquid as they gain enough kinetic energy to escape the surface of the liquid?
Bumek [7]
Im pretty sure They freeze
7 0
3 years ago
Read 2 more answers
The atomic number of arsenic is 33 what is the electron configuration
rjkz [21]
It is really easy if you look up an electron configuration table (one that looks like a periodic table) and then just go down the rows left to right, top to bottom, and just stop when you get to where the element is on the table.

 1s^2 2s^2 2p^{6}  3s^2 3p^6 4s^2 3d^1^0 4p^3
8 0
3 years ago
A barium hydroxide solution is prepared by dissolving 2.06 g of Ba(OH)2 in water to make 32.9 mL of solution. What is the concen
navik [9.2K]

Answer:  1.36 M

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

Molarity=\frac{n\times 1000}{V_s}

where,

n = moles of solute

To calculate the moles, we use the equation:

moles of solute= \frac{\text {given mass}}{\text {molar mass}}=\frac{2.06g}{171g/mol}=0.0120moles

Molarity=\frac{0.0120\times 1000}{32.9}=0.364M

The balanced reaction between barium hydroxide and perchloric acid:

2HCIO_4+Ba(OH_)2\rightarrow BaCIO_4+2H_2O

To calculate the concentration of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is HClO_4

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is Ba(OH)_2

We are given:

n_1=1\\M_1=?\\V_1=8.50mL\\n_2=2\\M_2=0.364M\\V_2=15.9mL

Putting values in above equation, we get:

1\times M_1\times 8.50=2\times 0.364\times 15.9\\\\M_1=1.36M

Thus the concentration of the acid is 1.36 M

4 0
3 years ago
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