Given the following mixture of two compounds 45.00 g of X (MW =78.00 g/mol)(density 1.128 g/mL) and 610.00 mL of Y (62.00 g/mol))(density 0.872 g/mL), calculate the mole fraction of X.
1. Given the following mixture of two compounds 45.00 g of X (MW =78.00 g/mol)(density 1.128 g/mL) and 610.00 mL of Y (62.00 g/mol))(density 0.872 g/mL), calculate the mole fraction of X.
2. Given the following mixture of two compounds 25.00 mL of X (MW =87.00 g/mol)(density 1.077 g/mL) and 620.00 mL of Y (90.00 g/mol))(density 1.229 g/mL). The boiling point of pure Y is -3.00 degrees C. The molal boiling constant is 3.276 degrees C/m. What is the boiling point of the solution.
3. Given the following mixture of two compounds 35.00 mL of X (MW =75.00 g/mol)(density 0.879 g/mL) and 765.00 mL of Y (74.00 g/mol))(density 1.161 g/mL). The vapor pressure of pure Y is 24.00. Calculate the vapor pressure of the solution.
4. 3.82 grams of a water soluble ionic compound with the formula of A1X4 (Molar mass of 125.00 grams/mol) is dissolved in 64 grams of water. Calculate the expected boiling point of the solution. The boiling point elevation constant for water is 0.512 degrees C/molal. The boiling point of water is 99.20 degrees C.
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