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lead-204 203.973amu, 1.40% abundance. lead-206 205.974 amu, 24.10% abundance. lead-207???, abundance 22.10%. lead-208 207.977, abundance 52.40%. Calculate the isotope mass of lead-207
=207.2 amu (Pb)
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205 gram hydrogen sulfide reacts with 75.0 g oxygen to produce sulfur and water. Find: a) Gram of sulfur formed b) gram of excess reactant used up c) gram of excess reactant that remained unreacted
H2S + O2 --->>H2O + SMolar mass of H2S = 34.1= 205/34.1 = 6.0112 molesMolar mass of oxygen = 31.99875/31.998 = 2.344 molesMole ratio in both cases = 1:1= 2.344+6.0112...
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Write an equation to represent the decomposition of lead (IV) sulfide into lead metal and solid sulfur. What is reduced? What is oxidized?
PbS = Pb + SPb+2 converts into Pb0 - it is reducedS-2 converts into S0 - it is oxidized
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if 27 grams of copper II sulfide reacts with 22 grams of sodum nitrate how many grams of sodium sulfide can be formed
CuS + NaNO3 → Cu(NO3)2 + Na2S – no reaction! This reaction between these substances is not possible, because copper II sulfide not dissociates into ions in water, and probable...
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Mercuric sulfide, HgS, contains 82.6% mercury by mass. What mass of mercuric sulfide
can be prepared from 60.0 g of mercury?
The 60.0 g of mercury is 82.6% of mercuric sulfide, than the mass of all mercuric sulfide is 100%. The mass of mercuric sulfide (g) = (60.0g/82.6%)*100% = 72.6 g....
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A lead atom has a mass of 3.4 x 10 g neg 22 power. How many lead atoms are in a cube of lead that has a volume of 7.00cm to the 3rd power if the density of lead is 11.3g/cm to the 3rd power
1 . ᵽ = m/V, m = ᵽ * V m = 7*11,3 = 79,1g 2 . N = m/ma = 79,1/34*10⁻²² = 23,265*10²²
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You conducted an experiment in the lab that involves the reaction of silver (Ag) with sulfur (S). You used 0.018g of silver with excess sulfur and produced 0.0150g of silver sulfide (Ag2S).
You conducted an experiment in the lab that involves the reaction of silver (Ag) with sulfur (S). You used 0.018g of silver with excess sulfur and produced 0.0150g of silver...
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solid zinc reacts with gaseous sulfur and yields solid zinc (II) sulfide.
Equation:
Type of reaction:
Question #87466Equation: 3Zn + SO2 = ZnS + 2ZnOType of reaction: Ion exchange
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5kg of potassium is reacted with excess sulfur to make potassium sulfide. Work out the mass of potassium sulfide produced.
128.2 mole x mole2K + S -> K2S2 mole 1 molen(K) = m(K)/M(K) = 5 000 g/39 g/mole = 128.2 mole128.2 mole/2 mole = x mole/1 molex = (128.2 *...
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