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3 years ago

You use 4.98 g of Na2SO4, how many grams of barium sulfate are produced? Na2+Ba(NO3)2= ?

Chemistry

1 answer:

Kaylis [27]3 years ago

6 0

Answer:

Mass of barium sulfate = 8.17 g

Explanation:

Given data:

Mass of sodium sulfate = 4.98 g

Mass of barium sulfate produced = ?

Solution:

Na₂SO₄ + Ba(NO₃)₂ → BaSO₄ + 2NaNO₃

Moles of sodium sulfate:

Number of moles = mass/molar mass

Number of moles =4.98 g / 142.04 g/mol

Number of moles = 0.035 mol

Now we will compare the moles pf sodium sulfate and with barium sulfate.

Na₂SO₄ : BaSO₄

1 : 1

0.035 : 0.035

Mass of barium sulfate:

Mass = number of moles × molar mass

Mass = 0.035 mol ×233.4 g/mol

Mass = 8.17 g

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An oxide of phosphorus contains 56.4% phosphorus and 43.6% oxygen. It's relative molecular mass is 220. Find both the empirical

sladkih [1.3K]

Moles of P = 56,4g/30,974g/mole = 1,82 moles P
moles of O = 43,6/15,999 = 2,73 moles of O

converting to the simplest ratio:
For P : 1,82/1,82 = 1
For O : 2,73/1,82 = 1,5

1 P and 2 oxygens.
PO2 -> the empirical formula

hope this help

7 0

3 years ago

Read 2 more answers

he rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy . If the rate c

Leya [2.2K]

The question is incomplete, here is the complete question:

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea = 71.0 kJ/mol . If the rate constant of this reaction is 6.7 M^(-1)*s^(-1) at 244.0 degrees Celsius, what will the rate constant be at 324.0 degrees Celsius?

<u>Answer:</u> The rate constant at 324°C is $61.29M^{-1}s^{-1}$

<u>Explanation:</u>

To calculate rate constant at two different temperatures of the reaction, we use Arrhenius equation, which is:

$\ln(\frac{K_{324^oC}}{K_{244^oC}})=\frac{E_a}{R}[\frac{1}{T_1}-\frac{1}{T_2}]$

where,

$K_{244^oC}$ = equilibrium constant at 244°C = $6.7M^{-1}s^{-1}$

$K_{324^oC}$ = equilibrium constant at 324°C = ?

$E_a$ = Activation energy = 71.0 kJ/mol = 71000 J/mol (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314 J/mol K

$T_1$ = initial temperature = $244^oC=[273+244]K=517K$

$T_2$ = final temperature = $324^oC=[273+324]K=597K$

Putting values in above equation, we get:

$\ln(\frac{K_{324^oC}}{6.7})=\frac{71000J}{8.314J/mol.K}[\frac{1}{517}-\frac{1}{597}]\\\\K_{324^oC}=61.29M^{-1}s^{-1}$

Hence, the rate constant at 324°C is $61.29M^{-1}s^{-1}$

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4 years ago

(c) O2 gas is transferred from a 3 L vessel containing oxygen at 4 atm to an evacuated 20 L vessel at a constant temperature of

Fudgin [204]

Answer:

After the transfer the pressure inside the 20 L vessel is 0.6 atm.

Explanation:

Considering O2 as an ideal gas, it is at an initial state (1) with V1 = 3L and P1 = 4 atm. And a final state (2) with V2 = 20L. The temperature remain constant at all the process, thus here applies the Boyle-Mariotte law. This law establishes that at a constant temperature an ideal gas the relationship between pressure and volume remain constant at all time:

$P x V = k$

Therefore, for this problem the step by step explanation is:

$P_{1} xV_{1} = P_{2} xV_{2}$

Clearing P2 and replacing

$P_{2}= \frac{P_{1} xV_{1}}{V_{2} } = \frac{4atmx3L}{20L} = 0.6atm$

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3 years ago

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loris [4]

Probably the diamond pickaxe

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3 years ago

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Iron Choose one: A. is alloyed with carbon and chromium to make stainless steel. B. was the first of the common metals (iron, al

Lostsunrise [7]

Answer:

A. is alloyed with carbon and chromium to make stainless steel.

Explanation:

Steel is an alloy formed mainly of iron and carbon but some other metals like chromium are also added in little amounts.

Is steel, the percentage of iron and carbon together is about 90% and the rest metals fall in the 10% part.

Although the cost of steel is low, it has a very high tensile strength and that's why it is used in tools, ships, buildings, trains and in various types of infrastructures.

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3 years ago