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3 years ago

Compared to an electron, which particle has a charge that is equal in magnitude but opposite in sign?

1 answer:

8 0

I think the correct answer is proton since protons have a charge of +1 while electrons have a charge of -1. However, since beta particles are used to name a type of nuclear decay and can refer to either a positron or electron depending on the circumstances, your teacher might want you to put beta particle since positrons are basically electrons but that have a positive charge.
I hope this helps. Let me know if anything is unclear.

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When 5.00 g of Al2S3 and 2.50 g of H2O are reacted according to the following reaction: Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H

Debora [2.8K]

Answer:

$Y=58.15\%$

Explanation:

Hello,

For the given chemical reaction:

$Al_2S_3(s) + 6 H_2O(l) \rightarrow 2 Al(OH)_3(s) + 3 H_2S(g)$

We first must identify the limiting reactant by computing the reacting moles of Al2S3:

$n_{Al_2S_3}=5.00gAl_2S_3*\frac{1molAl_2S_3}{150.158 gAl_2S_3} =0.0333molAl_2S_3$

Next, we compute the moles of Al2S3 that are consumed by 2.50 of H2O via the 1:6 mole ratio between them:

$n_{Al_2S_3}^{consumed}=2.50gH_2O*\frac{1molH_2O}{18gH_2O}*\frac{1molAl_2S_3}{6molH_2O}=0.0231mol Al_2S_3$

Thus, we notice that there are more available Al2S3 than consumed, for that reason it is in excess and water is the limiting, therefore, we can compute the theoretical yield of Al(OH)3 via the 2:1 molar ratio between it and Al2S3 with the limiting amount:

$m_{Al(OH)_3}=0.0231molAl_2S_3*\frac{2molAl(OH)_3}{1molAl_2S_3}*\frac{78gAl(OH)_3}{1molAl(OH)_3} =3.61gAl(OH)_3$

Finally, we compute the percent yield with the obtained 2.10 g:

$Y=\frac{2.10g}{3.61g} *100\%\\\\Y=58.15\%$

Best regards.

7 0

3 years ago

Borax (na2b4o7Â·10h2o; fw = 381.372 g/mol; density = 1.73 g/ml), a primary standard, was used to standardize a solution of hno3.

SashulF [63]

<span>0.06355391 mol The balanced equation for the reaction is Na2B4O7*10H2O + 2 HNO3 = 2 NaNO3 + 4 H3BO3 + 5 H2O So for each mole of Borax to neutralize, it takes 2 moles of HNO3. Calculate number of moles of Borax 0.2619 g / 381.372 g/mol = 0.0006867 mol Moles of HNO3 used = 0.0006867 mol * 2 = 0.0013734 mol Molarity is defined as moles per liter so divide the number of moles used by the volume in liters. So 0.0013734 / 0.02161 = 0.06355391 mol</span>

3 0

4 years ago

Por favor, necesito ayuda, es urgente!!!

PilotLPTM [1.2K]

Answer:

what type of language this is ??

4 0

3 years ago

What is the bond between a posative and a negative ion called

guajiro [1.7K]

Answer:

Your answer would be Ionic bond.

5 0

3 years ago

How do you find the equilibrium constant?

Blababa [14]

Answer:

we find the chemical equilibrium constant by balancing the number of reactant and products

Explanation:

and after balancing using formula (KC) = Ratio of product / reactants

8 0

3 years ago