Predict the direction of reaciton in equilibirum in each case:
a. KClO3 (s) ---- KCl (s) + O2 (g) **IF pressure is
increased?
b. 3 A (g) + B (s) ---- 2C (g) **IF pressure is decreased?
a) If pressure is increased, the reaction will move in that direction where the number of moles of gaseous reactants are less. so the reaction will move in reverse direction that is towards reactants.
b) If pressure is decreased, the reaction will move in that direction where the number of moles of gaseous reactants are more. so the reaction will move in reverse direction that is towards reactants.
Predict the direction of reaciton in equilibirum in each case: a. KClO3 (s) ---- KCl (s)...
You are given 2.773 g of a mixture of KClO3 and KCl. When heated, the KClO3 decomposes to KCl and O2, 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g), and 803 mL of O2 is collected over water at 22 °C. The total pressure of the gases in the collection flask is 751 torr. What is the weight percentage of KClO3 in the sample? The formula weight of KClO3 is 122.55 g/mol. The vapor pressure of water...
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?
C12H22O11(s) + 8 KClO3(s) -> 12 CO2(g) + 11 H2O(g) + 8 KCl(s) KClO3 = 122.6 g/mol sucrose = 342.3 g/mol CO2 = 44.01 g/mol 1 skittle = 0.84 grams of sucrose 1. If each skittle contains 0.84 g of sucrose (C12H22O11) What is the minimum number of skittles needed to maximize the product (no KClO3 remaining) if I use 12.0 g of KClO3?
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...
C12H22O11(s) + 8 KClO3(s) -----> 12 CO2(g) + 11 H2O(g) + 8 KCl(s) KClO3= 122.6 g/mol sucrose= 342.3 g/mol CO2= 44.01 g/mol 1 skittle= .84 grams of sucrose 1. If each skittle contains 0.84 g of sucrose (C12H22O11) What is the minimum number of skittles needed to maximize the product if I use 12.0g of KClO3? 2. How many grams of reactant remain (excess) after 2.5g of sucrose and 25.0g KClO3 react? 3. If 2.2 grams of CO2 are produced,...
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.
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)
C12H22O11(s) + 8 KClO3(s) -> 12 CO2(g) + 11 H2O(g) + 8 KCl(s) KClO3 = 122.6 g/mol sucrose = 342.3 g/mol CO2 = 44.01 g/mol 1 skittle = 0.84 grams of sucrose ** 17.85 (g) remaining of KCLO3- reactant ** 5 skittles from sucrose If 2.2 grams of CO2 are produced, what is the percent yield?
Balance the following equation KClO3 → KCl + O2 The sum of the coefficients is 5 6 7 13 Which one of the compounds is polar ? Electronegativity H = 2.1 Electronegativity C = 2.5 Electronegativity N = 3.0 Electtronegativity Cl = 3.0 Electronegativity O = 3.5 CH4 CCl4 NH3 CO2 Balance the following redox reaction the coefficient in front of OH- is Zn + NO3- → Zn2+ + NH3 ( basic solution) 3 4 8 9 Calculate the density of CO2 gas...