A 15.0 g sample of hydrated copper sulfate was heated to dryness and the new mass measured to be 9.59 g. Calculate the percentage of water in the hydrated crystal with the correct number of significant figures.
A) 63%
B) 63.3%
C) 36.1%
D) 45%
E) 36%
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A 15.0 g sample of hydrated copper sulfate was heated to dryness and the new mass...
Question 2 3 pts A 15.0 g sample of hydrated copper sulfate was heated to dryness and the new mass measured to be 9.59 g. Calculate the percentage of water in the hydrated crystal with the correct number of significant figures. 63% 36.1% 36% 63.3% 45% Question 3 2 pts When correctly balanced, the coefficients for the following equation are: NH3(g) + _O2(g) → __NO(g) + __H20 (g) None of these. O 2, 2, 2,2 O 2,3,2,3 4,5,4,6 O 5,3,5,4
A 0.551-g sample of hydrated copper(II) sulfate, CuSO4.xH2O, was heated carefully until it had changed completely to anydrous copper(II) sulfate (CuSO4) with a mass of 0.308 g. Determine the value of x. [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit of copper(II) sulfate in the hydrated crystal.
A hydrated form of copper sulfate (CuSO4⋅?H2O) is heated to drive off all of the water. If there is initially 7.28 g of hydrated salt and there is 4.07 g of anhydrous CuSO4 after heating, find the number of water molecules associated with each CuSO4 formula unit. x = ?
A hydrated form of copper sulfate (CuSO4 xH,O) is heated to drive off all of the water. If there is initially 9.22 g of hydrated salt and there is 5.89 g of anhydrous CuSo, after heating, find the number of water molecules associated with each CUSO4 formula unit.
A 1.803-g sample of gypsum, a hydrated salt of calciumsulfate, CaSO4, is heated in a crucible until a constantmass is reached. The mass of the anhydrous CaSO4 salt is1.426-g. Calculate the percent by mass of water in the hydratedcalcium sulfate salt. Also, calculate the moles of water removedand the moles of anhydrous CaSO4 remaining in thecrucible. And, finally, What is the formula of the hydrated calciumsulfate; that is, what is the whole-number mole ratio of calciumsulfate to water? Please show...
Mass of evaporating dish (g) Mass of evaporating dish and hydrated sample Mass of original hydrated sample (g) Mass of evaporating dish and dehydrated 40 , 31 41. 34g sample (g) Mass of dehydrated sample (g) Mass of water evolved (g) Mass of evaporating dish and copper (g) Mass copper (g) Mass of chlorine (g) 6.349 40,し39 0 37g DATA ANALYSIS 1. How many moles of water were in your sample of copper chloride hydrate? (Show calculations). H 1.01 x...
A student heated a sample of a hydrated salt and obtained the following data: Grams of hydrated salt used: 1.0000 gram Grams of anhydrous salt (147 g/mole) recovered: 0.8033 grams Grams of water vapour (18 g/mole) lost: 0.1967 grams Determine the percentage by mass of water in this hydrate. (1) How many water molecules, "X", are bonded to this hydrated salt, salt. X H20? (2)
When a 7.50 g sample of hydrated LiClO, is heated to drive off all the water, the anhydrous residue that remains has a mass of 4.97 g. What is the mass percent of water in the hydrate?
4. When a 7.50 g sample of hydrated LiClo, is heated to drive off all the water, the anhydrous residue that remains has a mass of 4.97 g. What is the mass percent of water in the hydrate?
5) The total mass of a crucible and some copper(II) sulfate hydrate in the cruible was 34.567 g. The crucible (with copper (II) sulfate hydrate in it was heated at 110 °C for 30 minutes. And the total mass decreased to 33.125 g. How many grams of mass was lost during heating? B) 1.44g A) 1.4420g C) 18 D) 1.4g E) 1.442g 6) Assuming that all are measured quantities, complete the following operation and express the result in the correct...