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3 years ago

At 189k a sample of gas has a volume of 32.0cm. what does the gas occupy at 242k

Chemistry

1 answer:

sattari [20]3 years ago

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<h2>Answer:</h2>

At 189 K volume = 32.0 cm

As volume of gas is directly proportional to temperature.

As the temperature increase the volume of gas will also increase.

Volume at 1 K = 32/189

Volume at 242 K = 32/189 * 242 = 40.97 cm.

Gas occupy 40.97 cm volume at 242 K.

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An exothermic reaction has a positive enthalpy (heat) of reaction.(T/F)

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Answer:

True.

Explanation:

An exothermic reaction has a positive enthalpy (heat) of reaction. However, it can be negative in some circumstances.

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3. Two people are playing tug of war. One person pulls to the right with 32 N of force. The other person pulls to the left with

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The net force = -5 N

The direction : to the left(negative sign)

<h3>Further explanation </h3>

Net force : the sum of all forces acting on an object

Force is a vector quantity that has both magnitude and direction,

We agree that the move up and to the right is a positive sign, while down and to the left is a negative sign.

The direction of the force (horizontal motion) is to the right (+32 N), and to the left (-37 N), so the net force :

$\tt \sum F=F~right-F~left\\\\\sum F=32-37\\\\\sum F=-5~N$

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Chlorine. Electronegativity generally increases up and across the periodic table

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I’m not sure what the answer is

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I believe it’s the third option
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Burning 12.00 g of an oxoacid produces 17.95 g of carbon dioxide and 4.87 g of water. Consider that 0.25

Veseljchak [2.6K]

Answer: The molecular formula will be $C_6H_6O_6$

Explanation:

Mass of $CO_2$ = 17.95 g

Mass of $H_2O$ = 4.87 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 17.95 g of carbon dioxide, = $\frac{12}{44}\times 17.95=4.89g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 4.87 g of water, = $\frac{2}{18}\times 4.87=0.541g$ of hydrogen will be contained.

Mass of oxygen in the compound = (12.00) - (4.89+0.541) = 6.57 g

Mass of C = 4.89 g

Mass of H = 0.541 g

Mass of O = 6.57 g

Step 1 : convert given masses into moles.

Moles of C = $\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{4.89g}{12g/mole}=0.407moles$

Moles of H= $\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.541g}{1g/mole}=0.541moles$

Moles of O= $\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{6.57g}{16g/mole}=0.410moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{0.407}{0.407}=1$

For H = $\frac{0.541}{0.407}=1$

For O = $\frac{0.410}{0.407}=1$

The ratio of C : H : O = 1: 1 : 1

Hence the empirical formula is $CHO$ .

Hence the empirical formula is $CHO$

The empirical weight of $CHO$ = 1(12)+1(1)+1(16)= 29 g.

If 0.25 moles has mass of 44.0 g

Thus 1 mole has mass of = $\frac{44.0}{0.25}\times 1=176g$

Thus molecular mass is 176 g

Now we have to calculate the molecular formula.

$n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{176g}{29g}=6$

The molecular formula will be= $6\times CHO=C_6H_6O_6$

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3 years ago