In a lab experiment, 8.24 g of phosphorus reacts with bromine to form 72.01 g of phosphorus tribromide.
(a) Calculate the percentage by mass of P in phosphorus tribromide.
(b) How many grams of bromine reacted?
How do you know?
law of definite proportions
law of multiple proportions
law of constant composition
law of conservation of mass
In a lab experiment, 8.24 g of phosphorus reacts with bromine to form 72.01 g of...
In a lab experiment, 7.75g of phosphorus reacts with bromine to form 67.68g of phosphorus tribromide a) Calculate the percentage by mass of P in phosphorus tribromide b) How many grams bromine reacted and how do you know?
In a lab experiment, 6.3 g of Mg reacts with sulfur to form 14.6 g of magnesium sulfide. (a) Use the equation below to calculate the percentage by mass of Mg in magnesium sulfide. % X component amount of component x 400 total amount (b) How many grams of sulfur reacted? How do you know? law of constant composition law of conservation of mass law of definite proportions law of multiple proportions Need Help?
In a lab experiment, 6.9 g of Mg reacts with sulfur to form 16.0 g of magnesium sulfide. (a) Use the equation below to calculate the percentage by mass of Mg in magnesium sulfide. % X component = amount of component x.. total amount 4.9 % (b) How many grams of sulfur reacted? 49 How do you know? O law of constant composition O law of definite proportions O law of multiple proportions O law of conservation of mass
ShipPS14 12 E.009 . Ask Your Tes -/5 points My Notes 0/6 Submissions Used In a lab experiment, 5.6 g of Mg reacts with sulfur to form 13.0 g of magnesium sulfide. (a) Use the equation below to calculate the percentage by mass of Mg in magnesium sulfide amount of component X %X component 100% total amount 40 (b) How many grams of sulfur reacted? 40 How do you know? law of conservation of mass law of multiple proportions law...
Phosphorus tribromide decomposes to form phosphorus and bromine, like this: 4 PBr() - P.(o) + 6 Brz() Also, a chemist finds that at a certain temperature the equilibrium mixture of phosphorus tribromide, phosphorus, and bromine has the following composition: PBr compound pressure at equilibrium 30.2 atm P. 35.1 atm Bry 50.2 atm Calculate the value of the equilibrium constant for this reaction. Round your answer to 2 significant digits. x 5 ?
If 0.419 g of hydrogen is obtained in this experiment, how many grams of sulfur must be obtained? What fundamental law does this experiment demonstrate? -Law of Multiple Proportions -Law of Definite Proportions -Conservation of Mass
Phosphorus and liquid bromine react vigorously together to form phosphorus tribromide. P4 +6Br24 PBrz If 5.Og of phosphorus and 35g of bromine react, how many grams of PBr3 could be produced? Oa) 5 g PBrz Ob) 39.5 g PBr3 Oc) 79 g PBr3 Od) 0.146 g PBr3
Nitrogen reacts with bromine to form the molecular compound NBr3. Nitrogen and phosphorus are in the same group. In Chapter 4 we learned about reactivity and groups. What compound would you expect to form if phosphorus reacted with bromine? A) PBT B) PBr2 C) PBr3 D) PBr4
In a lab experiment, 5.2 g of Mg reacts with sulfur to form 12.1 g of magnesium sulfide. How much magnesium sulfide would be formed if 5.2 g of Mg were reacted with 13.8 g of S? How many g?
1.A 12.39g sample of phosphorus reacts with 45.4 g of Chlorine to form Phosphorus Trichloride(PCl3). if it PCL3 is the only product, what is the mass of pcl3 formed? 2.Determine the molarity of a solution formed by dissolving 8.47g LiBr in enough water to yield 750 mL of solution 3. Calculate the mass percent composition of Oxygen Al2(SO4)3