Answer: 4.18925 kJ heat is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50°C.
Explanation:
Temperature of Solid
Melting temperature of Solid ![C_2H_5OH=114^oC=159 K](https://tex.z-dn.net/?f=C_2H_5OH%3D114%5EoC%3D159%20K)
Temperature of liquid ![C_2H_5OH=-50^oC=223K](https://tex.z-dn.net/?f=C_2H_5OH%3D-50%5EoC%3D223K)
Specific heats of solid ethanol = 0.97 J/gK
Specific heats of liquid ethanol = 2.3 J/gK
Heat required to melt the the 25 g solid
at 159 K
= 159 K - 138 K = 21 K
![Q_1=mc\Delta T= 25\times 0.97J/gK\times 21 K=509.25 J](https://tex.z-dn.net/?f=Q_1%3Dmc%5CDelta%20T%3D%2025%5Ctimes%200.97J%2FgK%5Ctimes%2021%20K%3D509.25%20J)
Heat required to melt and raise the temperature of
upto 223 K
= 223 K - 159 K = 64 K
![Q_2=mc\Delta T= 25\times 2.3J/gK\times 64 K=3680 J](https://tex.z-dn.net/?f=Q_2%3Dmc%5CDelta%20T%3D%2025%5Ctimes%202.3J%2FgK%5Ctimes%2064%20K%3D3680%20J)
Total heat to convert solid ethanol to liquid ethanol at given temperature :
(1kJ=1000J)
Hence, 4.18925 kJ of heat will be required to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50°C.
Answer:
for the reaction is 18.05
Explanation:
Equilibrium constant in terms of partial pressure (
) for this reaction can be written as-
![K_{p}=\frac{P_{NO_{2}}^{2}}{P_{N_{2}O_{4}}}](https://tex.z-dn.net/?f=K_%7Bp%7D%3D%5Cfrac%7BP_%7BNO_%7B2%7D%7D%5E%7B2%7D%7D%7BP_%7BN_%7B2%7DO_%7B4%7D%7D%7D)
where
and
are equilibrium partial pressure of
and
respectively
Hence
= 18.05
So,
for the reaction is 18.05
<span>A chemist adds 155.0ml of a 4.10 X 10^-5 mmol/L of a zinc oxalate (ZnC2O4)solution to a reaction flask. Calculate the mass in micrograms of zinc oxalate the chemist has added to the flask.
1mmol = 10^-3 mol
Therefore 4.10*10^-5mmol = 4.10*10^-8mol
molar mass ZnC2O4 = 65.39+(2*12.011)+(4*15.99) = 153.372g/mol
You have 4.10*10^-8 mol/litre =153.372 * 4.10*10^-8 = 6.29*10^-6 grams / litre (* see below)
But you have 155ml. Mass of ZnC2O4 = 155/1000*6.29*10^-6 g
Mass is = 9.75*10^-7 grams
1µg = 10^-6 g
You then have 9.75*10^-7/10^-6 = 0.975µg ZnC2O4
(*see below) at this point you could have said:
1µg = 10^-6 g therefore you have a solution of 6.29µg per litre,
155ml = 6.29*155/1000 = 0.975µg ZnC2O4</span>
45 molecules of chlorine gas (Cl₂) are needed to react with 30 atoms of aluminum (Al)
The balanced equation for the reaction is given below:
2Al + 3Cl₂ —> 2AlCl₃
From the balanced equation above,
2 atoms of Al required 3 molecules of Cl₂.
With the above information, we can determine the number of molecules of Cl₂ needed to react with 30 atoms of Al. This can be obtained as follow:
From the balanced equation above,
2 atoms of Al required 3 molecules of Cl₂.
Therefore,
30 atoms of Al will require =
= 45 molecules of Cl₂.
Thus, 45 molecules of chlorine gas (Cl₂) are needed to react with 30 atoms of aluminum (Al)
Learn more: brainly.com/question/24918379