a mineral contains only a metal and sulfur. If analysis indicates that a 3.36 g sample of the mineral contains 1.39 g of lead, what is the mass fraction of lead in the mineral?
mass fraction of lead= mass of lead/mass of the mineral
mass fraction of lead=1.39/3.36 = 0.41369
a mineral contains only a metal and sulfur. If analysis indicates that a 3.36 g sample...
Fluorite, a mineral of calcium, is a compound of the metal with fluorine. Analysis shows that a 2.60 g sample of fluorite contains 1.67 g calcium. Calculate the following. (a) mass of fluorine in the sample g (b) mass fraction of calcium and fluorine in fluorite calcium fluorine (c) mass percent of calcium and fluorine in fluorite calcium % fluorine %?
Lead metal can be extracted from a mineral called galena, which contains 86.6%% lead by mass. A particular ore contains 68.5%% galena by mass. Part A If the lead can be extracted with 92.5%% efficiency, what mass of ore is required to make a lead sphere with a 7.00 cmcm radius? Express your answer with the appropriate units.
Lead metal can be extracted from a mineral called galena, which contains 86.6% lead by mass. A particular ore contains 68.5% galena by mass. Part A If the lead can be extracted with 92.5% efficiency, what mass of ore is required to make a lead sphere with a 5.00 cm radius? Express your answer with the appropriate units.
A 2.5600g sample of a compound that contains sulfur is analyzed by precipitating all the sulfur as BaSO4. If 1.1756 g of BaSO4 are obtained in the analysis, what is the percentage of sulfur in the original compound?
A 0.500-g sample of chromium metal reacted with sulfur powder to give 0.963 g of product. a) The mass of sulfur that reacted is _____ b) The empirical formula of the chromium sulfide is _____
Combustion analysis 12.01 g of an unknown sample, which
contains only carbon, hydrogen and oxygen, produced 14.08 g co2 and
4.32 h2o. Determine the empirical formula and molecular formula of
the unknown sample, while the molar mass for the unknown sample is
150.078 g/mol.
15 pts) Combustion analysis 12.01 g of an unknown sample, which contains only carbon, hydrogen, and oxygen, roduced 14.08 g CO2 and 4.32 g H20. Determine the empirical formula and molecular formula of the unknown sample,...
5. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of prod Calculate the empirical formula of the iron sulfide.6. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.861 g of product Calculate the empirical formula of the iron sulfide.
A chemical analysis of a water sample indicates that the water contains 6.50 times 10^-4 grams of Mercury metal per 2.00 liters of water. Convert the measurement to parts per million(ppm).Type in your answer without units.
6) A sample of a sulfide of a metal M, (formula MxSy), is submitted to analysis to identify the metal. The sulfur in the sample is recovered as 120 mL of 0.250 M Na2S solution. The metal in the same sample is recovered as 40.0 mL of 0.500 M solution of the metal ion. a. Find the formula MxSy of this metal sulfide. b. The molar mass of this sulfide is 150 g/mole. Identify the metal The final answer for...
A 1.000-g sample of cobalt metal reacted with sulfur powder to give 1.548 g of product. Record your numbers to 3 significant figures. Do not use exponential notation or subscripts in your answers. a) The mass of sulfur used in the reaction is b) The number of moles of cobalt is moles and the number of moles of sulfur is moles. c) Using their ratio of number of moles, the empirical formula of the cobalt sulfide is Draw the Lewis...