Chemistry

Chemistry, 29.08.2019 02:30, zach8782

Heating zinc sulfide in the air causes the formation of

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Chemistry, 10.07.2019 05:30, fireyking19

A100−g sample of zinc sulfide contains 67.1 g zinc and 32.9 g sulfur. if a 1.19−g sample of zinc is heated with excess sulfur, 1.77 g of zinc sulfide forms. are these data in agreement with the law of definite proportions?

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Chemistry, 21.08.2019 05:30, emmareese2022

The best explanation for the dissolution of zns in dilute hcl is that a. the sulfide ion concentration is decreased by the formation of h2s. b. the zinc ion is amphoteric. c. the zinc ion concentration is decreased by the formation of a chloro complex. d. the sulfide ion concentration is decreased by oxidation to sulfur. e. the solubility product of zncl2 is less than that of zns.

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Chemistry, 02.10.2019 20:30, Amandarobersonn

Zinc metal is produced by heating solid zinc sulfide with solid wine witte resulting in liquid zinc and sulfur dioxide gas write a balanced equation for the reaction using complete formulas for the compounds with phase labels (use the lowest possible coefficients. use the pull down boxes to specify states such as (aq) or (b). if a box is not needed, leave it blank.) submit answer try another version item attempts remaining

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Chemistry, 29.10.2019 04:31, 21ghostrider21

The first step in the process used to recover zinc metal from zinc sulfide ore is the reaction of zinc sulfide with oxygen gas to produce zinc oxide and sulfur dioxide. 2zns(s) 3o2(g)⟶2zno(s) 2so2(g) when the external pressure is 1.523×105 pa and the temperature is 675 k, the amount of work performed is 850.1 j. calculate how many grams of oxygen are consumed in the reaction.

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