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2 years ago

12

A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of and a temperature of 100.0°C. The unknown g

as is ________.

1 answer:

Zepler [3.9K]2 years ago

8 0

Answer:

Xenon

Explanation:

Step 1: Given data

Mass (m): 1.44 g

Volume (V): 0.335 L

Pressure (P): 1.00 atm (I looked it up)

Temperature (T): 100.0°C

Step 2: Convert the temperature to Kelvin

K = °C + 273.15 = 100.0°C + 273.15 = 373.2 K

Step 3: Calculate the number of moles (n)

We will use the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1.00 atm × 0.335 L / (0.0821 atm.L/mol.K) × 373.2 K

n = 0.0109 mol

Step 4: Calculate the molar mass of the gas

M = 1.44 g / 0.0109 mol = 132 g/mol

Step 5: Identify the gas

The gas with a molar mass of about 132 g/mol is xenon.

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Mashutka [201]

Answer:

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Explanation:

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assuming degree of dissociation $\alpha$ =1/10;

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and equation is;

$K_a = {c\alpha \times \alpha}$

$[H^{+}] = c\alpha$ = $\frac{K_a}{\alpha}$

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$P_H =-logK_a + log\alpha$

$K_a =1.38\times10^{-4}$

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2 years ago

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MAVERICK [17]

The correct reaction equation is:

$3NaHCO_{3} (aq) + C_{6}H_{8}O_{7} (aq) \rightarrow 3CO_{2} (g) + 3H_{2}O (l) + Na_{3}C_{6}H_{5}O_{7} (aq)$

Answer:

b) 1 mole of water is produced for every mole of carbon dioxide produced.

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a) <u>22.4 L of $CO_{2}$ gas</u> is produced only when <u> $\frac{22.4}{3}$ L of $C_{6}H_{8}O_{7}$ </u> is reacted with 22.4 L of $NaHCO_{3}$ . So it is wrong.

b) Since in the chemical equation the stoichiometric coefficient of $CO_{2}$ and $H_{2}O$ are same so the number of moles or volume of each of them will be same whatever the amount of reactants taken. <u>Therefore it is correct option.</u>

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2 years ago

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