In the decomposition of Ni_{2}O_{3} into nickel and oxygen, what would be the mass of residue (to three decimal places) remaining after heating, assuming that you started with 1.035g Ni_{2}O_{3}?
In the decomposition of Ni2O3 into nickel and oxygen, what would be the mass of residue...
Percentage of Oxygen in Potassium Chlorate Introduction: The thermal decomposition of potassium chlorate can be described by the following equation: 2 KCIO3(s) 2 KCls) + 3 O2(g) Egn 1 (D stands for heating, elevated temperature) In this experiment you will determine the percentage of oxygen in potassium chlorate. You will compare the experimental result with the theoretical percentage calculated from the formula KCIO3. While potassium chlorate decomposes simply by heating, the reaction is very slow. A catalyst is used. Catalyst...
Question 5 Status: Not yet answered | Points possible: 1.00 Suppose that you decompose 24.45 g of Ni2O3, which has a molar mass of 165.39 g/mol, into nickel and oxygen. 2 Ni203 (s) + 4 Ni (s) + 3 02 (g) After completing the decomposition, you have 9.14 g of solid Ni, which has a molar mass of 58.963 g/mol. What is the percent yield of your decomposition? Answer:
Sample 2 97.79 g 102.95 g 101.15 g Sample 1 (a) Mass of 98.32 g crucible + lid (b) Mass of crucible, lid + 103.76 g KCIO3 (c) Mass of crucible, lid + 102.01g residue after 1st heating (d) Mass of crucible, lid + residue after 101.69 g 2nd heating (e) Mass of crucible, lid + 101.68 g residue after 3rd heating 101.05 g 101.01 g Data Analysis .Use your data to determine the experimental mass percent of oxygen in...
After Heating .320 g of NaSO4•xH2O,The residue has a mass of .140g. Calculate the percentage of water in the hydrate. Write the hydrate formula 3. After heating,0320 g of Na2S04 Hydrate XH20, the residue has a mass of o, 140 g. Calculate the percentage (%) of water in the hydrate. What is the hydrate formula?
What mass of oxygen gas can be produced by the decomposition of 3.5 g of KClO3? Note: Your answer is assumed to be reduced to the highest power possible.
Question 4 Status: Not yet answered Points possible: 1.00 Consider the balanced equation of KI reacting with Pb(NO3), to form a precipitate. 2 KI (aq) + Pb(NO3)2 (aq) + Pbl (8) + 2 KNO3(aq) What mass of Pbl, can be formed by adding 0.489 L of a 0.364 M solution of KI to a solution of excess Pb(NO3)2? Answer: Question 5 Status: Not yet answered Points possible: 1.00 Suppose that you decompose 24.45 g of Ni 03, which has a...
2. Using the data from the experiment, calculate the mass of copper (II) sulfate residue and the mass of water (Items 5 and 6 from the Data Form). Express your answers in grams to the nearest hundredth (+ 0.01 g). Show your work. 3. Calculate the moles of copper (II) sulfate present from the mass of the copper (II) sulfate. Express your answer in moles as three significant digits. Show your work. 4. Calculate the moles of water driven off...
For the following reactions, what chemical reactions would you observe? 1) Butane and Oxygen 2) Decomposition of Ammonium Carbonate 3) Zinc and Citric Acid 4) Zinc Acetate and Sodium Phosphate Tribasic 5) Hydrochloric Acid and Potassium Carbonate
A metal alloy contains 15.7 % nickel (m/m)%. What mass of the metal alloy would contain 40.0 g of nickel?
New at this..clear steps would be great. A compound of mercury and oxygen is heated in order to decompose the compound. a 4.08g sample of mercury oxide upon heating gives off oxygen gas. After heating the mass of mercury metal left behind was 3.78g. calculate empirical formula of the compound.