2 years ago

Please help and thank you so much

Chemistry

1 answer:

olchik [2.2K]2 years ago

8 0

A. Sorry if I’m wrong :(

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Scorpion4ik [409]

Answer:

1.06 atm

Explanation:

We are given the following variables to work with:

Initial pressure (P1): unknown

Initial temperature (T1): 348 K

Final temperature (T2): 506 K

Final pressure (P2): 1.55 atm

We are asked to find the initial pressure (P1). We want to choose a gas law equation that relates initial pressure and temperature to final pressure and temperature. Gay-Lussac's law does this:

$\frac{P_{1}}{T_1} =\frac{P_{2}}{T_2} \\$

We can rearrange the law algebraically to solve for $P_{1}$ .

${P_{1}} =\frac{(T_1)(P_{2} )}{T_2} \\$

Substitute your known variables and solve:

${P_{1}} =\frac{(348 K)(1.55 atm )}{506 K} \\ = 1.06 atm$

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Answer:

The number of moles of AlBr3 = Molarity × Volume

= 0.400 × 0.700

= 0.28 moles

1 mole of AlBr3 gives 3 moles of Br- ions

That is

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Therefore, 0.045 moles of AlBr3 will yield 3 × 0.28 = 0.84 moles

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