Na2XO3(aq) + CaCl2(aq) →CaXO3(s) + 2NaCl(aq)
A total of 5.4842 grams of CaXO3 were collected. What is the identity of the element “X?”
A 5.6780 gram sample of the compound Na2XO3 was dissolved in water then reacted with excess...
A 4.1286 gram sample of the compound NaXPO3 was dissolved in water then reacted with excess copper nitrate: 2NaXPO3(aq) + XCu(NO3)2(aq) →CuX(PO3)2(s) + 2XNaNO3(aq) A total of 4.8639 grams of CuX(PO3)2 were collected. What is the value of X?
A 0.5187-gram sample of calcium chloride (CaCl2;MW 110.98g/mol) was dissolved in 300. mL of water. What is the molality of the solution? (Assume the density of water is 1.00g/ml)
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...
1.000 gram of compound A burns in excess oxygen (i.e., compound A is completely reacted) and yield 3.083 g of CO2 and 1.419 g of H2O a)What is the mass of hydrogen in 1.000 g of compound A? b)What is the mass percentage of hydrogen in compound A? c)Does compound A contain any other element(s)? For part a, i tried entering two values i got, 0.4 and 0.14, both were wrong. Can someone please explain how to solve this in...
A 0.5 gram sample of calcium chloride dihydrate (CaCl2 • 2H2O) is heated driving off the water. The dehydrated calcium chloride (CaCl2) weighs 0.38 grams. What was the % H2O by mass? Hint: Just use grams, there is absolutely no need for moles this time. It is not a trick question.
A 31.2 gram sample of C6H6 (benzene) is reacted with excess HNO3 (nitric acid). 36.0 grams of the desired product, nitrobenzene C6H5NO2, is isolated from this reaction. Water is the by-product. A. Write a balanced chemical equation for this reaction B. What is the percent yield of nitrobenzene?
Consider if 2.00g of alum were dissolved in water at a neutral pH and then reacted with a slight excess of sodium hydroxide as such: Al3+ (aq) + 3OH- (aq) ---> Al(OH)3 (s) What mass of aluminium hydroxide is formed?
When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0 C to 38.7 C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 0.710 mol of calcium chloride dissolves in water? The solution process is CaCl2(s) --> Ca2+(aq) + 2Cl–(aq)
A 2.00 g sample of silver nitrate is dissolved in water and then reacted with 0.250 g of copper metal, according to the reaction below. Answer the questions about this process. 2 AgNO3 (aq) + Cu (s) --> Cu(NO3)2 (aq) + 2 Ag (s) What mass of the excess reactant remains after the reaction goes to completion? (I want to see if you guys get this correct because I have no idea how to approach because it doesn't tell us...
A 1.42 g sample of a pure compound, with formula M_2SO_4, was dissolved in water and treated with an excess of aqueous barium chloride, resulting in the precipitation of all the sulfate ion as barium sulfate. The precipitate was collected, dried, and found to weigh 2.3.3 g. Determine the atomic mass of M, and identify M.