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riadik2000 [5.3K]
4 years ago
13

In the chemical reaction: 2 NaCl (s) + Pb(NO3)2 (aq) ---> 2 NaNO3 (aq) + PbCl2 (s), a student adds 2.5 grams of NaCl(s) to ex

cess lead (II) nitrate solution. What is the theoretical mass, in grams, of the precipitate (solid) formed
Chemistry
1 answer:
lakkis [162]4 years ago
4 0
The amount of the precipitate PbCl2 can be obtained using stoichiometry, assuming the reaction goes into completion given the excess amounts of the lead (II) nitrate solution. First, divide 2.5 g NaCl to its MW of 58.44 g/ mol to obtain the moles of NaCl involved in the reaction. Second, knowing that for every 2 moles of NaCl, there is 1 mole of PbCl2 produced, we divide the moles of NaCl obtained earlier by 2 to get the moles of PbCl2 produced. From the moles of PbCl2, we multiply it to its MW of 278.1 g/ mol. The amount of precipitate is then calculated to be 5.9484 g PbCl2. 
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Answer:

\°C=5.8x10^3\°C

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Explanation:

Hello,

In this case, for the calculation of the temperature in degree Celsius we subtract 273.15 to the given temperature in kelvins:

\°C=6100-273.15\\\\\°C=5.8x10^3\°C

Next, by applying the following equation we compute it in degree Fahrenheit:

\°F=(5.8x10^{3}*9/5) + 32\\\\\°F=1.1x10^4\°F

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julsineya [31]

Answer:

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Answer:

Explanation:

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