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Elina [12.6K]
3 years ago
5

A reaction has ∆H = −356 kJ and ∆S = −36 J/K. Calculate ∆G (kJ) at 25°C.

Chemistry
1 answer:
Cloud [144]3 years ago
5 0

Answer: -345.2 KJ

Explanation: As we know that ,dG=dH-TdS

T=25+273=298 K

dG= -356 x1000-298(-36)= -356000+10728

=-345272 j

= -345.2 KJ

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A 0.3832-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in oxygen to yield 0.7120 g of CO2
xxTIMURxx [149]

Answer:

C_3H_3O_2

Explanation:

Hello,

In this case, since the law of conservation of mass allows us to notice that the mass of carbon in the burned compound is also present in the resulting carbon dioxide, we can compute such moles as shown below:

n_C=0.7120gCO_2*\frac{1molCO_2}{44gCO_2} *\frac{1molC}{1molCO_2} =0.0162molC

Next, hydrogen in the sample is present at the products in the water only, and in one mole of water, two moles of hydrogen are present, thereby:

n_H=0.1458gH_2O*\frac{1molH_2O}{18gH_2O}*\frac{2molH}{1molH_2O}=0.0162molH

Nevertheless, the amount of oxygen in the sample must be computed by subtracting both the mass of carbon and hydrogen from the previously computed moles:

m_O=0.3832g-0.0162molC*\frac{12gC}{1molC} -0.0162molH*\frac{1gH}{1molH} =0.1726gO

And the moles:

n_O=0.1726gO*\frac{1molO}{16gO} =0.0108molO

Next, we compute the mole ratios with respect to the element having the smallest number of moles (oxygen) to obtain the subscripts in the empirical formula:

C=\frac{0.0162}{0.0108}=1.5\\ \\H=\frac{0.0162}{0.0108}=1.5\\\\O=\frac{0.0108}{0.0108}=1

Then, we have:

C_{1.5}H_{1.5}O_1

Finally, by multiplying by two, we obtain the smallest whole subscripts:

C_3H_3O_2

Best regards.

5 0
3 years ago
Which formula can be used to calculate the molar mass of ammonia (NH3)?
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<u>Answer:</u> The correct answer is Option C.

<u>Explanation:</u>

Molar mass is defined as the sum of the atoms present in a compound each multiplied with the number of atoms present in it.

For a compound A_xB_y

The molar mass will be = [(x\times \text{Molar mass of A})+(y\times \text{Molar mass of B})]

So, for the given compound NH_3,

The molar mass will be = [(1\times \text{Molar mass of Niyrogen})+(3\times \text{Molar mass of Hydrogen})]

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Answer:

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