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arsen [322]
3 years ago
13

An experiment is performed on a puck on a level air hockey table, where friction is negligible. a constant horizontal force is a

pplied to the puck, and the puck's acceleration is measured. now the same puck is transported far into outer space, where both friction and gravity are negligible. the same constant force is applied to the puck (through a spring scale that stretches the same amount), and the puck's acceleration (relative to the distant stars) is measured. what is the puck's acceleration in outer space?
Chemistry
1 answer:
motikmotik3 years ago
3 0
<span>Since friction is the only force dampening the acceleration of the puck, the acceleration of the puck in outer space will be equal to the acceleration on a hockey table where friction is negligible.</span>
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Explanation:

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If 0.896 g of a gas occupies a 250 mL flask at 20°C and 760 mm Hg of pressure, what is the molar mass of the gas?​
salantis [7]

Answer:

86.2 g/mol

Explanation:

Before you can find the molar mass, you first need to calculate the number of moles of the gas. To find this value, you need to use the Ideal Gas Law:

PV = nRT

In this equation,

-----> P = pressure (mmHg)

-----> V = volume (L)

-----> n = moles

-----> R = Ideal Gas constant (62.36 L*mmHg/mol*K)

-----> T = temperature (K)

After you convert the volume from mL to L and the temperature from Celsius to Kelvin, you can use the equation to find the moles.

P = 760 mmHg                                      R = 62.36 L*mmHg/mol*K

V = 250 mL / 1,000 = 0.250 L              T = 20 °C + 273.15 = 293.15 K

n = ? moles

PV = nRT

(760 mmHg)(0.250 L) = n(62.36 L*mmHg/mol*K)(293.15 K)

190 = n(18280.834)

0.0104 = n

The molar mass represents the mass (g) of the gas per every 1 mole. Since you have been given a mass and mole value, you can set up a proportion to determine the molar mass.

\frac{?grams}{1 mole} =\frac{0.896grams}{0.0104moles}                                      <----- Proportion

?grams(0.0104moles) = 0.896                       <----- Cross-multiply

?grams = 86.2                                               <----- Divide both sides by 0.0104

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How many moles of hydrochloric acid are required to produce .40 moles of hydrogen gas?

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Hydrogen gas = H2

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Cl = 1-

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2:1:1

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