Two hypothetical ionic compounds are discovered with the chemical formulas XCl2 and YCl2, where X and Y represent symbols of the imaginary elements. Chemical analysis of the two compounds reveals that 0.25 mol XCl2 has a mass of 100.0 g and 0.50 mol YCl2has a mass of 125.0 g.
a. What are the molar masses of XCl2 and YCl2?
b. If you had 1.0-mol samples of XCl2 and YCl2, how would the number of chloride ions compare?
c. If you had 1.0-mol samples of XCl2 and YCl2, how would the masses of elements X and Y compare?
d. What is the mass of chloride ions present in 1.0 mol XCl2 and 1.0 mol YCl2?
e. What are the molar masses of elements X and Y? I know that:
X = 100.00g – Cl2 = 100.00g - (35.453g*2) = 100.00g – 70.906g = 29.094g * 4 = 116.376g
Y = 125.0g – Cl2 = 125.00g - (35.453g*2) = 125.00g – 70.906g = 54.094g * 2 = 108.188g
is that it?
f. How many moles of X ions and chloride ions would be present in a 200.0-g sample of XCl2?
g. How many grams of Y ions would be present in a 250.0-g sample of YCl2?
h. What would be the molar mass of the compound YBr3?
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