Suppose you had a 95 g piece of sulfur
WebNov 21, 2015 · For oxygen, you will have. 32.72g ⋅ 1 mole O 16.0g = 2.045 moles O. To determine the empirical formula of the iron oxide, you need to find the smallest whole number ratio that exists between the two elements in the compound. To do that ,divide both values by the smallest one. For Fe: 1.534moles 1.534moles = 1. For O: 2.045moles … WebSuppose that 0.323 g of an unknown sulfate salt is dissolved in 50 mL of water. The solution is acidified with 6 M \(\ce{HCl}\), heated, and an excess of aqueous \(\ce{BaCl2}\) is slowly added to the mixture resulting in the formation of a white precipitate.
Suppose you had a 95 g piece of sulfur
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WebWhat net charge would you place on a 100 g piece of sulfur if you put an extra electron on 1 in 10 12 of its atoms? (Sulfur has an atomic mass of 32.1.) Expert Solution & Answer ... Ch. 18 - Considering Figure 18.46, suppose that qa= qdand... Ch. 18 - If qa = 0 in Figure 18-46, under what conditions... Ch. 18 - In regions of low humidity, one ... WebSuppose you had a 125 g piece of sulfur. What net charge, in coulombs, would you place on it if you put an extra electron on 1 in 10 12 of its atoms? (Sulfur has an atomic mass of 32.1) Q = Expert Answer Solution: Net charge Q=ne Where n= nu … View the full answer Previous question Next question
Web(a) Cu = 63.55 g (c) S = 32.07 g (b) Hg = 200.59 g (d) He = 4.00 g. Solution. Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro’s number of atoms for each of the following elements: (a) Copper (c) sulfur (b) Mercury (d) helium WebSep 30, 2024 · Your answer should be between 0.3 and 0.4 g (if you have a larger number than this, you are including the mass of the beaker). The masses recorded on Page 33 in Section I, part (c) include the mass of the containers (the mass of the empty containers is recorded in Section I, part (b)). ... Suppose you had three 1.000 g samples of magnesium ...
WebPercent yield represents the ratio between what is experimentally obtained and what is theoretically calculated, multiplied by 100%. #"% yield" = ("actual yield")/("theoretical yield") * 100%# So, let's say you want to do an experiment in the lab. You want to measure how much water is produced when 12.0 g of glucose (#C_6H_12O_6#) is burned with enough oxygen. WebWhat net charge would you place on a 100-g piece of sulfur if you put an extra electron on 1 in 10 12 of its atoms? (Sulfur has an atomic mass of 32.1 u.) Expert Solution & Answer ... Ch. 5 - Suppose you place a charge q near a large metal... Ch. 5 - Would defining the charge on an electron to be...
WebWe must know that an atom is composed of electrons, protons and neutrons. Th electrons are found in the orbits, the protons are found in the nucleus along with the protons. We could add a net charge to the electron by adding or removing an electron from it.
WebJul 19, 2024 · Suppose that a solution was prepared by dissolving 25.0 g of sugar into 100.0 g of water. The mass of the solution is mass of solution = 25.0g sugar + 100.0g water = 125.0 g The percent by mass would be calculated by: Percent by mass = 25.0 g sugar 125.0 g solution × 100 % = 20.0 % sugar Example 13.5. 1 brave little toaster watch onlineWebLet's say you have a radioactive isotope that undergoes radioactive decay. It started from a mass of 67.0 g and it took 98 years for it to reach 0.01 g. Here's how you would determine its half-life: Starting from (1), we know that 0.01 = 67.0⋅ (1 2)98.0 t1/2 → 0.01 67.0 = 0.000149 = ( 1 2)98.0 t1/2 98.0 t1/2 = log0.5(0.000149) = 12.7 brave little toaster weirdbrave little toaster w 158WebThe overall chemical equation says that 1 mole of glucose reacts with 6 moles of oxygen gas for the reaction to occur. So the glucose to oxygen ratio is 1:6, or basically we need 6 times as many moles of oxygen gas as we do glucose for the reaction to happen. So 0.129 x 6 = 0.833 moles of oxygen. Hope that helps. brave little toaster with bombWebJan 31, 2024 · It's ca. 18.015 g/mol. Convert the volume of the water to its mass, assuming that the density of pure water is 998 kg/m³: m = 6 l × 998 kg/m³ = 0.006 m³ × 998 kg/m³= 5.988 kg. It's easier to work with grams, so convert the mass: 5.988 kg = 5988 g. As you already know how the grams to moles conversion work, find the number of moles: brave little toaster womp bomp a lu bompWebScience Physics Suppose you had a 110 g piece of sulfur. What net charge, in coulombs, would you place on it if you put an extra electron on 1 in 1012 of its atoms? (Sulfur has an atomic mass of 32.1) Suppose you had a 110 g piece of sulfur. brave little toaster watch fullWebIf one piece is placed above another, the repulsive force can be great enough to support the top piece's weight. Assuming equal point charges (only an approximation), calculate the magnitude of the charge if electrostatic force is great enough to support the weight of a 10.0 mg piece of tape held 1.00 cm above another. brave little toaster voice cast