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zaharov [31]
3 years ago
5

A chemist needs 1.36 mol of strontium bromide, SrBr2, for a reaction. What mass of strontium chloride should the chemist use?

Chemistry
2 answers:
yaroslaw [1]3 years ago
5 0
Mass SrBr2 = 247.42 g/mol x 1.36 mol 
<span>= 336 g</span>
a_sh-v [17]3 years ago
4 0

Answer: 336.5 grams

Explanation:

According to avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number 6.023\times 10^{23} of particles.

convert given masses into moles.

Number of Moles =\frac{\text{ given mass}}{\text{ molar mass}}

Given number of moles = 1.36

Molar mass of SrBr_2 = 247.43 g/mol

Putting in the values we get

1.36=\frac{\text {given mass}}{247.43g/mole}

{\text {given mass}}=336.5grams

Thus mass of strontium bromide used should be 336.5 grams.

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A scientist fills a large, tightly sealed balloon with 75,000 mL of helium at STP.
pav-90 [236]

Considering the definition of STP conditions, 3.35 moles of helium are contained within the balloon.

<h3>Definition of STP condition</h3>

The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.

<h3>Amount of moles of helium within the balloon</h3>

In this case, you know that scientist fills a large, tightly sealed balloon with 75,000 mL of helium at STP.

So, you can apply the following rule of three: if by definition of STP conditions 22.4 liters are occupied by 1 mole of helium, 75 L (75 L= 75000 mL, being 1 L= 1000 L) are occupied by how many moles of helium?

amount of moles of helium=\frac{75 Lx1 mole}{22.4 L}

<u><em>amount of moles of helium= 3.35 moles</em></u>

Finally, 3.35 moles of helium are contained within the balloon.

Learn more about STP conditions:

brainly.com/question/26364483

brainly.com/question/8846039

brainly.com/question/1186356

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