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3 years ago

8

For the reaction below, Kp = 1.59 at 100°C. If 1.0 g of SrCO3 is placed in an empty 5.00 L reactor and allowed to reach equilibr

ium, what will be the pressure in the reactor?

1 answer:

Sergio [31]3 years ago

8 0

Answer:

$p_{CO_2}^{eq}=1.59atm$

Explanation:

Hello, in this case, one could consider the undergoing chemical reaction as:

$SrCO_3(s)\rightleftharpoons SrO(s)+CO_2(g)$

Thus, since 1.0 g of strontium carbonate is placed, the equilibrium equation takes the following form, excluding the solid-stated species and considering just the carbon dioxide as it is gaseous:

$Kp=p_{CO_2}^{eq}=1.59atm$

Hence, since at the beginning there is no carbon dioxide, its pressure at equilibrium equals Kp:

$Kp=p_{CO_2}^{eq}=1.59atm$

Which was clearly defined above.

Best regards.

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If the density of a 45.0 cm3 block of wood is 0.65 g/ml what is the mass of the wood?

wlad13 [49]

Answer:

$\boxed {\tt mass=29.25 \ grams}$

Explanation:

The density formula is mass over volume.

$d=\frac{m}{v}$

Rearrange the formula for the mass, m. Multiply both sides of the formula by v.

$d*v=\frac{m}{v}*v$

$d*v=m$

Mass can be found by multiplying the density and volume. The density is 0.65 grams per milliliter and the volume is 45.0 cubic centimeters.

A cubic centimeter is equal to a milliliter.

Therefore, 45 cubic centimeters also equals 45 milliliters.

$d= 0.65 \ g/mL\\v= 45 \ mL$

Substitute the values into the formula.

$0.65 \ g/mL * 45 \ mL=m$

Multiply. Note the milliliters, or mL will cancel out.

$0.65 \ g * 45=m$

$29.25 \ g=m$

The mass of the wood is 29.25 grams.

5 0

3 years ago

0.254g lead(ii)ethanoate, on adding excess K2CrO4 solution, gave 0.130g of lead(ii)chromate precipitate. what is the percentage

Alborosie

Answer:

32.8%

Explanation:

All of the Pb⁺² species precipitated as lead(II) cromate, PbCrO₄ (we know this as excess K₂CrO₄ was used).

First we convert 0.130 g of PbCrO₄ into moles, using its molar mass:

0.130 g ÷ 323 g/mol = 4.02x10⁻⁴ mol PbCrO₄

There's 1 Pb⁺² mol per PbCrO₄ mol, so in total 4.02x10⁻⁴ moles of Pb⁺² were in the ethanoate sample.

We <u>convert those 4.02x10⁻⁴ moles of Pb into grams</u>:

4.02x10⁻⁴ mol * 207 g/mol = 0.083 g Pb

Finally we calculate the percentage composition of Pb:

0.083 g Pb / 0.254 g salt * 100% = 32.8%

3 0

3 years ago

Determine the wavelength of the energy that needs to be absorbed for a 3p electron in chlorine to be promoted to the 4s subshell

bazaltina [42]

Answer:

The wavelength of the energy that needs to be absorbed = 52.36 nm

Explanation:

For this study;

Let consider the Rydgberg equation from Bohr's theory of atomic model:

i.e.

$\dfrac{1}{\lambda} = R_H (Z^*)^2( \dfrac{1}{n_1^2}-\dfrac{1}{n_2^2})$

where

Z* = effective nuclear charge of atom = Z - σ = 6

n₁ = lower orbit = 3

n₂ = higher orbit = 4

$R_H$ = Rydyberg constant = 1.09 × 10⁷ m⁻¹

λ = wave length of the light absorbed

∴

$\dfrac{1}{\lambda} = 1.09 \times 10^7}(6)^2( \dfrac{1}{3^2}-\dfrac{1}{4^2})$

$\dfrac{1}{\lambda} = 1.09 \times 10^7}(36)( \dfrac{1}{9}-\dfrac{1}{16})$

$\dfrac{1}{\lambda} = 392400000\times0.0486111111$

$\dfrac{1}{\lambda} =19075000$

$\lambda = \dfrac{1}{19075000}$

$\lambda = \dfrac{1}{1.91\times 10^7 \ m^{-1}}$

$\lambda = 5.236 \times 10^{-8} m$

$\lambda = 52.36 \times 10^{-9} m$

$\lambda = 52.36\ n m$

Therefore, the wavelength of the energy that needs to be absorbed = 52.36 nm

7 0

3 years ago

Describe how this instrument works.<br><br> Operation:

Alex Ar [27]

Answer:

It amplifies the picture of something far away.

Explanation:

5 0

3 years ago

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In the following reaction: Ca+2 + 2Br- ---> BaBr2, which of the reactants is LEO and which is GER?

Makovka662 [10]

Chemical Reaction : Ca+2 + 2Br- ---- CaBr2

The answer: LEO is Bromine (Br-1); the oxidation state changes from (0 to -1) and GER is Calcium (Ca+2); the oxidation state changes from (0 to +2).

5 0

3 years ago