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4 years ago

Why is it necessary to mix the solution very rapidly when the bleach is added?

1 answer:

3 0

It is necessary to add the bleach rapidly because the chemical reaction will occur rapidly. In order to get all of the bleach to interact with the other substance as a whole and not in part, it is necessary to add everything in a very rapid manner, otherwise the amount of the other chemical may not have enough time to properly interact with all of the bleach.

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The gas begins with a temperature of 333 K and a pressure of 4.00 atm that increases to 7.65 atm as the gas is heated. What is t

blsea [12.9K]

The final temperature on increasing the pressure to 7.65 atm is 637 K.

Explanation:

The relation between temperature attained by gas molecules at varying pressure is defined by Guy-Lusac's law. It states that at constant volume, the pressure experienced by the gas molecules is directly proportional to the temperature attained by those molecules.

P∝T

Here, the initial pressure P₁ is given as 4 atm at temperature T₁ = 333 K, then the final pressure P₂ = 7.65 atm can be attained at temperature T₂.

The final temperature should be greater than the initial temperature as there is an increase in the pressure.

So,

$\frac{P_{1} }{T_{1} } = \frac{P_{2} }{T_{2} }$

$\frac{4}{333} =\frac{7.65}{T_{2} } \\\\T_{2} =\frac{7.65*333}{4} = 636.8 =637 K$

Hence, the final temperature on increasing the pressure to 7.65 atm is 637 K.

6 0

3 years ago

What minimum mass of iron (II) nitrate must be added to 10.0 of a 0.0699 M phosphate solution in order to completely precipitate

ad-work [718]

Answer: The minimum mass of iron (II) nitrate that must be added is 0.188 grams

Explanation:

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

Molarity of phosphate solution = 0.0699 M

Volume of solution = 10 mL = 0.010 L (Conversion factor: 1 L = 1000 mL)

Putting values in above equation, we get:

$0.0699M=\frac{\text{Moles of phosphate solution}}{0.010L}\\\\\text{Moles of phosphate solution}=(0.0699mol/L\times 0.010L)=6.99\times 10^{-4}mol$

The given chemical equation follows:

$2PO_4^{3-}(aq.)+3Fe(NO_3)_2(aq.)\rightarrow Fe_3(PO_4)_2(s)+6NO_3^-(aq.)$

By Stoichiometry of the reaction:

2 moles of phosphate solution reacts with 3 moles of iron (II) nitrate

So, $6.99\times 10^{-4}mol$ of phosphate solution will react with = $\frac{3}{2}\times 6.99\times 10^{-4}=1.049\times 10^{-3}mol$ of iron (II) nitrate

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of iron (II) nitrate = 180 g/mol

Moles of iron (II) nitrate = $1.049\times 10^{-3}$ moles

Putting values in above equation, we get:

$1.049\times 10^{-3}mol=\frac{\text{Mass of iron (II) nitrate}}{180g/mol}\\\\\text{Mass of iron (II) nitrate}=(1.049\times 10^{-3}mol\times 180g/mol)=0.188g$

Hence, the minimum mass of iron (II) nitrate that must be added is 0.188 grams

7 0

3 years ago

What happens after excitation in spectroscopy.

Bess [88]

Answer:

When a molecule is excited to a higher state it often ends up in its lowest excited state S1 and then emits radiation.

4 0

3 years ago

VOCABULARY 1. What is an ideal gas?

noname [10]

Answer:

a hypothetical gas whose molecules occupy negligible space and have no interactions, and which consequently obeys the gas laws exactly.

Explanation:

7 0

3 years ago

How many moles of NH3 have to be added to 1.0 L of water to dissolve 0.20 moles of AgCl?

d1i1m1o1n [39]

Not working on this yet

6 0

3 years ago