A mixture containing KClO3, K2CO3, KHCO3, and KCl was heated, producing CO2,O2, and H2O gases according to the following equations:
2KClO3(s)2KHCO3(s)K2CO3(s)→→→2KCl(s)+3O2(g)K2O(s)+H2O(g)+2CO2(g)K2O(s)+CO2(g)
The KCl does not react under the conditions of the reaction. 100.0 g of the mixture produces 1.70 g of H2O, 12.66 g of CO2, and 4.00 g of O2. (Assume complete decomposition of the mixture.)
You may want to reference (Page) Section 3.7 while completing this problem.
a. How many grams of KClO3 were in the original mixture?
Express your answer to three significant figures.
b. How many grams of KHCO3 were in the original mixture?
c. How many grams of K2CO3 were in the original mixture?
A mixture containing KClO3, K2CO3, KHCO3, and KCl was heated, producing CO2,O2, and H2O gases according...
A mixture of KCl and KClO3 weighing 1.40 g was heated; the dry O2 generated occupied 143 mL at STP. What percent by mass of the original mixture was KClO3, which decomposes as follows: 2KClO3(s) = 2KCl (s) + 3O2(g)
When heated, KClO3 decomposes into KCl and O2. 2KClO3⟶2KCl+3O2 If this reaction produced 83.4 g KCl, how many grams of O2 were produced? mass: g O2
When heated, KClO3 decomposes into KCl and O2. 2KClO3⟶2KCl+3O2 If this reaction produced 82.0 g KCl, how many grams of O2 were produced? mass: g O2
When heated, KClO3 decomposes into KC and O2. 2KClO3⟶2KCl+3O2 If this reaction produced 46.4 g KCl, how many grams of O2 were produced?
a 0.897 g mixture of solid KClO3 is heated. the KClO3 decomposes to KCl and O2. the mass after heating is 0.642 g. 2KClO=2KCl + 3 O2 a) how many grams of o2 is produced? b) what is the mass percentage of KClO in the mixture?
A mixture contains KClO3 and KCl. When the mixture is heated, only the KClO3 decomposes via the following reaction: 2KClO3 (s) → 3O2 (g) + 2KCl (s) In an experiment to determine the percent KClO3 in a KClO3/KCl mixture, the mixture was heated in a crucible several times in order to bring it to constant mass. The following experimental data was obtained. Before Heating Mass empty crucible + lid = 21.77 g Mass crucible + lid+ KClO3/KCl mixture = 26.16...
A mixture contains KClO3 and KCl. When the mixture is heated, only the KClO3 decomposes via the following reaction: 2KClO3 (s) → 3O2 (g) + 2KCl (s) In an experiment to determine the percent KClO3 in a KClO3/KCl mixture, the mixture was heated in a crucible several times in order to bring it to constant mass. The following experimental data was obtained. Before Heating Mass empty crucible + lid = 21.84 g Mass crucible + lid+ KClO3/KCl mixture = 26.19...
When heated, kCLO3 decomposes into KCL and O2. 2KCLO3 →2 KCI + 302 If this reaction produced 51.3 g KCI, how many grams of O2 were produced? When heated, KCIO, decomposes into KCl and 0,- 2KCIO, — 2 KCI +30, If this reaction produced 51.3 g KCl, how many grams of O, were produced? mass: mass: [ 80,
A 4.42 g sample of a KCl−KClO3 mixture is decomposed by heating and produces 147 mL O2(g), measured at 23.8 ∘C and 95.0 kPa . 2KClO3(1)→KCl(s)+3O2(g) What is the mass percent of KClO3 in the mixture? Express your answer to three significant figures.
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s). The equation for the reaction is 2KClO3⟶2KCl+3O2⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 48.8 g KClO3(s).