Explanation:
to calculate theoratical yield...first we must calculate how much Sucrose moles we have..in order to to do so...we must calculate molar mass of sucrose.
molar mass of sucrose is 342.3 g/mol.
now we can calculate how many sucrose moles we have by dividing the mass with molar mass of sucrose
735g/(342.3g/mol)=2.147mol
theoratically...according to stoichiometry..every 1 mole of sucrose yields 4 moles of ethanol...so...
2.147mole yield 2.147*4mol=8.588mol
now we must calculate weight of that much ethanol..molar mass of ethanol is 46.07 g/mol...
so we can multiple moles by molar mass to obtain the weight 8.588mol*46.07g/mol=395.649g
but we only obtained 310.5g...so percentage we have is
![\frac{310.5}{395.649} \times 100](https://tex.z-dn.net/?f=%20%5Cfrac%7B310.5%7D%7B395.649%7D%20%20%5Ctimes%20100)
78.47%
if there is trouble with molar mases I used....use what you calculated...
If my explanation is good enough...please mark it as brainliest.thanks
Answer:
The vapor pressure at 60.21°C is 327 mmHg.
Explanation:
Given the vapor pressure of ethanol at 34.90°C is 102 mmHg.
We need to find vapor pressure at 60.21°C.
The Clausius-Clapeyron equation is often used to find the vapor pressure of pure liquid.
![ln(\frac{P_2}{P_1})=\frac{\Delta_{vap}H}{R}(\frac{1}{T_1}-\frac{1}{T_2})](https://tex.z-dn.net/?f=ln%28%5Cfrac%7BP_2%7D%7BP_1%7D%29%3D%5Cfrac%7B%5CDelta_%7Bvap%7DH%7D%7BR%7D%28%5Cfrac%7B1%7D%7BT_1%7D-%5Cfrac%7B1%7D%7BT_2%7D%29)
We have given in the question
![P_1=102\ mmHg](https://tex.z-dn.net/?f=P_1%3D102%5C%20mmHg)
![T_1=34.90\°\ C=34.90+273.15=308.05\ K\\T_2=60.21\°\ C=60.21+273.15=333.36\ K\\\Delta{vap}H=39.3 kJ/mol](https://tex.z-dn.net/?f=T_1%3D34.90%5C%C2%B0%5C%20C%3D34.90%2B273.15%3D308.05%5C%20K%5C%5CT_2%3D60.21%5C%C2%B0%5C%20C%3D60.21%2B273.15%3D333.36%5C%20K%5C%5C%5CDelta%7Bvap%7DH%3D39.3%20kJ%2Fmol)
And
is the Universal Gas Constant.
![R=0.008 314 kJ/Kmol](https://tex.z-dn.net/?f=R%3D0.008%20314%20kJ%2FKmol)
![ln(\frac{P_2}{102})=\frac{39.3}{0.008314}(\frac{1}{308.05}-\frac{1}{333.36})\\\\ln(\frac{P_2}{102})=4726.967(\frac{333.36-308.05}{333.36\times308.05})\\\\ln(\frac{P_2}{102})=4726.967(\frac{25.31}{333.36\times308.05})\\\\ln(\frac{P_2}{102})=4726.967(\frac{25.31}{102691.548})\\\\ln(\frac{P_2}{102})=1.165](https://tex.z-dn.net/?f=ln%28%5Cfrac%7BP_2%7D%7B102%7D%29%3D%5Cfrac%7B39.3%7D%7B0.008314%7D%28%5Cfrac%7B1%7D%7B308.05%7D-%5Cfrac%7B1%7D%7B333.36%7D%29%5C%5C%5C%5Cln%28%5Cfrac%7BP_2%7D%7B102%7D%29%3D4726.967%28%5Cfrac%7B333.36-308.05%7D%7B333.36%5Ctimes308.05%7D%29%5C%5C%5C%5Cln%28%5Cfrac%7BP_2%7D%7B102%7D%29%3D4726.967%28%5Cfrac%7B25.31%7D%7B333.36%5Ctimes308.05%7D%29%5C%5C%5C%5Cln%28%5Cfrac%7BP_2%7D%7B102%7D%29%3D4726.967%28%5Cfrac%7B25.31%7D%7B102691.548%7D%29%5C%5C%5C%5Cln%28%5Cfrac%7BP_2%7D%7B102%7D%29%3D1.165)
Taking inverse log both side we get,
![\frac{P_2}{102}=e^{1.165}\\\\P_2=102\times 3.20\ mmHg\\P_2=327\ mmHg](https://tex.z-dn.net/?f=%5Cfrac%7BP_2%7D%7B102%7D%3De%5E%7B1.165%7D%5C%5C%5C%5CP_2%3D102%5Ctimes%203.20%5C%20mmHg%5C%5CP_2%3D327%5C%20mmHg)
The melting point of the solid form of water, which is ice, is 0°C. When we convert both temperatures to kelvin by adding 273 to each we get the melting point of copper as 1357K and that of ice is 273K. Then, dividing the melting point of copper by the melting point of ice, both in absolute temperature scale. The answer would be 4.97. Thus, the energy of molecules of copper is approximately 5 times compared to that of water.
Basaltic this is the answer