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18 Nov 2019

An element X has a triiodide with the empirical formula XI3 and a trichloride with the empirical formula XCl3. The triiodide is converted to the trichloride according to the equation

XI3 + Cl2-------->XCl3 + I2

If the complete conversion of 1.735 g of XI3 results in the formation of 0.904 g of XCl3, what is the atomic mass of the element X?

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Patrina Schowalter
Patrina SchowalterLv2
29 Mar 2019

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Related questions

2)Boron trichloride is prepared from the following reaction. 2B2O3 + 6Cl2 + 3C --> 4BCl3 + 3CO2 If 3.456g of B2O3 is mixed with 9.9216g of Cl2 and 2.459g of C then answer the following questions.

2a) What is the theoretical yield of boron trichloride in grams?

2b) How much of each of the excess reagents would remain once the reaction is complete? (report in grams)

3) If the yield of the reaction in question 2 is known to be only 67.89% using stochometric amounts, how much (g) of each of the three reagents would you need to obtain 10.000g of boron trichloride?


A sample of a substance with the empirical formula XBr3 weighs 0.5724 g. When it is dissolved in water and all its bromine is converted to insoluble AgBr by addition of an excess of silver nitrate, the mass of the resulting AgBr is found to be 1.1056 g. The chemical reaction is

XBr3 + 3 AgNO3 -----------> 3AgBr + X(NO3)3



(a) Calculate the formula mass of XBr3.

Formula mass XBr3 = g mol-1



(b) Calculate the atomic mass of X.

Atomic mass X = g mol-1

A sample of a substance with the empirical formula XBr2 weighs 0.5674 g. When it is dissolved in water and all its bromine is converted to insoluble AgBr by addition of an excess of silver nitrate, the mass of the resulting AgBr is found to be 0.9542 g. The chemical reaction is

XBr2 + 2 AgNO32AgBr + X(NO3)2

(a) Calculate the formula mass of XBr2.

Formula mass

XBr2 = g mol-1

(b) Calculate the atomic mass of X.

Atomic mass

X = g mol-1

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