In the following reaction, if there are 2.00 g of tin oxide to start with and excess hydrogen, what is the ratio between solid tin and water at equilibrium?

Booster class

General Chemistry 2

Skill

Relate equilibrium concentrations of reactants and products

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Irving HeathcoteLv2

1 Sep 2020

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Related questions

Tin reacts with nitric acid in a crucible to form tin nitrate. Heating the product of this reaction generates nitrogen dioxide, a brown gas, and tin oxide. Given the following experimental results, what is the formula of the tin oxide formed?

Mass of crucible = 13.457 g

Mass of crucible + tin = 14.710 g

Mass of crucible after heating = 15.048 g

marooncricket327

Tin metal (Sn) and purple iodine (I₂) combine to form orange, solid tin iodide with an unknown formula.

Sn metal + solid I₂ → solid Sn_xI_y

Weighed quantities of Sn and I₂ are combined, where the quantity of Sn is more than is needed to react with all of the iodine. After Sn_xI_y has been formed, it is isolated by filtration. The mass of excess tin is also determined. The following data were collected:

Mass of tin (Sn) in the original mixture 1.056 g

Mass of iodine (I₂) in the original mixture 1.947 g

Mass of tin (Sn) recovered after reaction 0.601 g

What is the empirical formula of the tin iodide obtained?

lilacant875

To find the empirical formula of tin oxide, you first react Tin metal with nitric acid in a porcelain crucible. The metal is converted to tin nitrate, but, on heating the nitrate strongly, brown nitrogen dioxide gas is evolved and tin oxide is formed. In the laboratory you collect the following data: