In a lab experiment, 8.21g of phosphorus reacts with bromine to form 71.75 g of phosphorus tribromide. (a) Calculate the percentage by mass of P in phosphorus tribromide. 4.0 11.44 % (b) How many grams of bromine reacted? 4.0 Enter a number with the correct number of significant figures. How do you know? O law of constant composition law of multiple proportions law of conservation of mass O law of definite proportions

In a lab experiment, 8.21g of phosphorus reacts with bromine to form 71.75 g of phosphorus tribromide. (a) Calculate the percentage by mass of P in phosphorus tribromide. 4.0 11.44 % (b) How many grams of bromine reacted? 4.0 Enter a number with the correct number of significant figures. How do you know? O law of constant composition law of multiple proportions law of conservation of mass O law of definite proportions

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 33E

See similar textbooks

Similar questions

Calculate the average density of a single Al-27 atom by assuming that it is a sphere with a radius of 0.143 nm. The masses of a proton, electron, and neutron are 1.67261024g,9.10941028g, and 1.67491024g, respectively. The volume of a sphere is 4r3/3, where r is its radius. Express the answer in grams per cubic centimeter. The density of aluminum is found experimentally to be 2.70 g/cm3. What does that suggest about the packing of aluminum atoms in the metal?
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1 volume gas X + 2 volumes gas Y 2 volumes compound I 2 volumes gas X + 1 volume gas Y 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
In Groups 4A-6A, there are several elements whose symbols begin with S. Name these elements, and for each one give its symbol, atomic number, group number, and period. Describe each as a metal, metalloid, or nonmetal.
The mole is the SI unit for the amount of a substance. The mass of one mole of pure table sugar is 342.3 grams. How many grams of sugar are in exactly 1/2 mole? What is the mass of 0.764 mole?
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1. volume gas X + 2 volumes gas Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
5.00 g of copper is reacted with 5.00 g of sulfur in a crucible and acompound composed of copper and sulfur is formed. If the copper was completely reacted and the mass of the compound is 6.26 g, how many grams of sulfur formsthe compound? Calculate the mass percentage of copper and sulfur, respectively, in the compound.
Samples of illicit “street” drugs often contain an inactivecomponent, such as ascorbic acid (vitamin C). After obtaining a sample of cocaine, government chemists calculate the mass ofvitamin C per gram of drug sample, and use it to track the drug’sdistribution. For example, if different samples of cocaine ob-tained on the streets of New York, Los Angeles, and Paris allcontain 0.6384 g of vitamin C per gram of sample, they very likely come from a common source. Do these street samplesconsist of a compound, element, or mixture? Explain
A sample of zinc sulfide having a mass of 3.04 g was analyzed and found tocontain 1.00 g of sulfur, and the remainder zinc. If a prospector discovered1000 kg of pure zinc sulfide, what would be the maximum amount of zinc thatcould be recovered?
Cocaine (C₁₇H₂₁O₄N) is a natural substance found in cocaleaves, which have been used for centuries as a local anestheticand stimulant. Illegal cocaine arrives in the United States eitheras the pure compound or as the hydrochloride salt(C₁₇H₂₁O₄NHCl). At 25C, the salt is very soluble in water(2.50 kg/L), but cocaine is much less so (1.70 g/L). (a) Whatis the maximum amount (in g) of the salt that can dissolve in50.0 mL of water? (b) If the solution in part (a) is treated withNaOH, the salt is converted to cocaine. How much additionalwater (in L) is needed to dissolve it?
Is there a difference between a homogeneous mixture of hydrogen and oxygen in a 2:1 ration and a sample of water vapor? Explain.
A student performed an experiment of heating a hydrate and obtained the following data. the mass of the empty crucible was 17.556g the mass of crucible and a hydrate was 21.018g the mass of the crucible and anhydrous salt ( after heating ) was 19.641g Calcualte the mass of the hydrated salt.
A certain alloy with a density of 11.5 g/cm3 contains 55% iron by mass. a) How many pg of iron would be present in a 4.5"x5.0"x11" piece of alloy?