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A copper wire with a mass of 4.32 g reacts with sulfur to form 5.41 g of a copper sulfide compound. a) Determine the number of moles of copper and sulfur in the compound. b) Determine the empirical formula of the product. c) If the actual formula of the sulfide compound contains 1 S, what is the molecular formula of the compound? d) Write the balance equation for the combination reaction.
Suppose the calorimeter for this experiment had been made of a heat-conducting material (such as metal) rather than plastic foam, so that the portion of heat energy lost to the calorimeter itself was larger and could not be ignored
If you wanted to prepare a solution of CO in water at 25 degrees Celsius in which the CO concentration was 2.5 mM, what pressure of CO would you need to use?
Draw the structure of the product that is formed when but-1-yne is treated with the following reagents:1) disiamylborane; 2) H2O2, KOH; 3) LiAlH4. Disiamylborane = [(i-Pr)(CH3)CH]2BH, a hindered derivative of BH3.
A voltaic cell consists of a strip of cadmium metal in a solution of Cd(NO3)2 in one beaker, and in the other beaker a platinum electrode is immersed in a NaCl solution
Consider a saturated colution of calcium oxalate, CaC2O4, in which the following reactions can occur: (CaC2O4)4 -2 (s) ---> Ca+2 + C2O4 -2 Ksp=1.3e-8
Identify the conjugate base of CH3COOH in the following reaction
Assume that the octet rule is followed for the N atom when you draw your structure(s). Pick the correct statement from the choices below.
Calculate the pH of a buffer solution obtained by dissolving 22.0 g of KH2PO4(s) and 36.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.
Using the following data, calculate the standard enthalpy of reaction for the coal gasification process 2C(s) + 2H2O(g) --> CH4(g) + CO2(g).
A sample of 1.00 mol of perfect gas molecules, originally at 1.00 atm, with a molar heat capacity at constant pressure of 7/2 R is put through the following cycle:
What magnitude of current is required to produce 1.0 kg of sodium metal in one hour by electrolysis?
The equation for the combustion of acetone is: 2 C3H6O + 8 O2 ---> 6 H2O + 6 CO2 + 852.6 kcal How much heat will be given off if 0.18 mol of acetone is completely burned?
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