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2 years ago

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A 1.0 L volume of gas at 27.0°C exerts a pressure of 85.5 K PA what will the pressure be at 127°C assume constant volume

1 answer:

Marianna [84]2 years ago

4 0

Answer:

114 kPa

Explanation:

Using Gay-Lussac's law you get the equation $\frac{P1}{T1} x \frac{P2}{T2}$ and converting celcius you get the final equation of $\frac{85.5}{27+273} x \frac{P2}{127+273}$ . After dividing 85.5 by 27+273(300) you get 0.285 and then you multiply 0.285 by 127+273 (400). You finally get 114 kPa

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Explanation:

1 mol of Ba(OH)2 = 2 moles of HCl

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3 years ago

What nuclide undergoes fission to form molybdenum-103, atomic number 42, tin-131, atomic number 50, and two neutrons?

FrozenT [24]

Answer:

The correct answer is Pu, 234.

Explanation:

In the given case, let us consider the reactant as X. Now the mass number (balanced) on both the sides will be,

Mass of X = Mass of Molybdenum + Mass of Tin + Mass of neutrons

M = 1 * 103 + 1 * 131 + 2 * 0

M = 234

Now the atomic number (balanced) on both the sides,

Atomic number of X = Atomic number of Molybdenum + Atomic number of Tin + Atomic number of neutrons

A = 1*42 + 1*50 + 2*1

A = 94

The atomic number 94 is for the element Plutonium, whose symbol is Pu. Thus, the reactant is 234-Pu.

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3 years ago

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Answer:

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Explanation:

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3 years ago

2HgCl2(aq) + C2O42–(aq) → 2Cl–(aq) +2CO2(g) + Hg2Cl2(s)

alexgriva [62]

Explanation:

Expression for rate of the given reaction is as follows.

Rate = k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y[/tex]

Therefore, the reaction equations by putting the given values will be as follows.

$1.8 \times 10^{-5} = k[0.105]x [0.15]y$ ............. (1)

$7.2 \times 10^{-5} = k [0.105]x [0.30]y$ ........... (2)

$3.6 \times 10^{-5} = k [0.0525]x [0.30]y$ ............ (3)

Now, solving equations (1) and (2) we get the value of y = 2. Therefore, by solving equation (2) and (3) we get the value of x = 1.

Therefore, expression for rate of the reaction is as follows.

Rate = $k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y$

Rate = $k [HgCl2]1 [C_{2}O^{-2}_{4}]2$

Hence, total order = 1 + 2 = 3

According to equation (1),

$1.8 \times 10^{-5} = k[0.105]x [0.15]y$

$1.8 \times 10^{-5} = k [0.105]1 [0.15]2$

k = $7.6 \times 10^{-3} M^{-2} min^{-1}$

Thus, we can conclude that rate constant for the given reaction is $7.6 \times 10^{-3} M^{-2} min^{-1}$ .

8 0

3 years ago