Question 11An 18 carat white gold is made by dissolving 12.5188 gof Copper, 14.1431 g of Silver, and 63.5172 g ofPalladium in 276.3933 g of Gold. What is the percentcomposition by mass of Silver in the metal alloy?Take note of the following values:• Density●• Ag = 10.5 g/mL• Au = 19.3 g/mLCu = 8.94 g/mL• Pd = 12.0 g/mL●●• Molar Mass• Ag = 107.87 g/molAu 196.97 g/mol=●Cu = 63.55 g/mol• Pd = 106.42 g/molRound your answer to 3 decimal places.

The percent composition by mass of silver in metal alloy is = 3.86 %

An 18 carat white gold is made by dissolving 12.5188 g of Copper, 14.1431 g of Silver, and 63.5172 g of Palladium in 276.3933 g of Gold. What is the percent composition by mass of Silver in the metal alloy?

An 18 carat white gold is made by dissolving 12.5188 g of Copper, 14.1431 g of Silver, and 63.5172 g of Palladium in 276.3933 g of Gold. What is the percent composition by mass of Silver in the metal alloy?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A student determined the mass of NaCl extracted during an experiment to be 0.42 grams. If the mass of the original mixture was 1.97 determine the percent of NaCl.
If 226.1 g of tin(II) chloride was the actual amount obtained in a reaction for which the theoretical yield was 288.0 g, the percentage yield is what?
In an experiment to determine the empirical formula of magnesium chloride, 0.50 g of magnesium ribbon was taken in a beaker and a few drops of HCl was added until all the Mg reacted with the acid liberating the hydrogen gas. The reaction completion was noted by observing that the bubbling stopped and no solid Mg was seen in the beaker. The beaker was heated to remove water and the dried magnesium chloride was weighed and found to be 1.99 g. What is the empirical formula for magnesium chloride based on this experiment?
If 31.0 g of MgSO4⋅7H2O is thoroughly heated, what mass of anhydrous magnesium sulfate will remain? Express your answer to three significant figures and include the appropriate units.
An impure sample of table salt (NaCl) that was dissolved in water and treated with silver nitrate to form silver chloride. If the initial sample had a mass of 1.741 g and the final mass of the AgCl was found to be 4.084 g, what is the mass percent of NaCl in the impure sample?
When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment, 1.50 g of copper was heated with excess sulfur to yield 1.64 g copper(I) sulfide. What is the percent yield?
When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment, 1.50 g of copper was heated with excess sulfur to yield 1.79 g copper(I) sulfide. What is the percent yield?
A sample of bismuth weighing 0.687 g was converted to bismuth chloride by reacting it first with HNO3, and then with HCI, followed by careful evaporation to dryness. The mass of the bismuth chloride obtained was 1.032 g. What is the empirical formula of bismuth chloride? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2.
5 g of hydrated barium chloride is heated in a crucible until the mass of the sample no longer changes. The mass of the sample after heating is 4.26 g. Assume that the mass lost during the heating is solely due to the loss of water from the sample. What percentage of water was contained in the barium chloride hydrate?
When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment, 1.50 g of copper was heated with excess sulfur to yield 1.80 g copper(I) sulfide. What is the percent yield?
50.0 g of tin(II) fluoride reacts with 50.0 g of sodium phosphate. Calculate the grams of tin(II) phosphate that would be formed in the reaction.
Your crucible has a mass of 30.074 g when empty, and does not change upon heating. You add some solid iron and then weigh the crucible and iron to be 32.860 g together. You then burn the iron in the presence of oxygen following the procedure in the handout. Assume that there are no contaminates and all of the iron is converted to iron oxide. The final mass of the crucible and iron oxide is 33.961 g, which does not change upon heating. The unrounded empirical formula obtained from these measurements would be FeOX, where X is a decimal type number (not necessarily a whole number). Give the value of X in the blank below in decimal format with the correct number of significant figures.Answer: ________