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4 years ago

Which gas law states that the pressure of a gas decreases when volume is increased and the temperature is unchanged

2 answers:

andrey2020 [161]4 years ago

4 0

Boyle's law state that the total pressure of an enclosed gas is inversely proportional to the volume of the container, as long as the temperature is constant

Nesterboy [21]4 years ago

3 0

Answer: Boyle's law

Explanation: It states that pressure of a gas is inversely proportional to the volume of a gas at constant temperature.

$P$ ∝ $\frac{1}{V}$ at constant temperature

or If the pressure of gas is decreased, the volume increases if the temperature is unchanged and If the pressure of gas is increased, the volume decreases if the temperature is unchanged.

$P_1V_1=P_2V_2$

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What is the total pressure exerted by a mixture of 48.0 grams of CH4 and 56.0 grams of

Oksi-84 [34.3K]

The pressure of the gas is obtained as 48 atm.

<h3>What is the total pressure?</h3>

Now we know that;

Number of moles of CH4 = 48.0 grams /16 g/mol = 3 moles

Number of moles of H2 = 56.0 grams/2 g/mol = 28 moles

Total number of moles present = 3 moles + 28 moles = 31 moles

Using;

PV =nRT

P = total pressure

V = total volume

n = total number of moles

R = gas constant

T = temperature

P = nRT/V

P = 31 * 0.082 * 286/15

P = 48 atm

Learn more about pressure of a gas:brainly.com/question/18124975

#SPJ1

4 0

1 year ago

The number of grams of H2 in 1470 mL of H2 gas.

Lorico [155]

Answer:

0.1313 g.

Explanation:

It is known that at STP, 1.0 mole of ideal gas occupies 22.4 L.

Suppose that hydrogen behaves ideally and at STP conditions.

<u><em>Using cross multiplication:</em></u>

1.0 mol of hydrogen occupies → 22.4 L.

??? mol of hydrogen occupies → 1.47 L.

∴ The no. of moles of hydrogen that occupies 1.47 L = (1.0 mol)(1.47 L)/(22.4 L) = 6.563 x 10⁻² mol.

Now, we can get the no. of grams of hydrogen in 6.563 x 10⁻² mol:

<em>The no. of grams of hydrogen = no. of hydrogen moles x molar mass of hydrogen</em> = (6.563 x 10⁻² mol)(2.0 g/mol) = <em>0.1313 g.</em>

5 0

3 years ago

After an electric sign is turned on, the temperature of its glass goes from 23.5°C to 65.5°C. The sign’s glass has a mass of 905

julia-pushkina [17]

The sign's glass absorbed 25466.7 J

<h3>Further explanation</h3>

Given

The temperature of glass : 23.5 °C to 65.5 °C

mass = 905 g

the specific heat capacity = 0.67 J/g °C

Required

Heat absorbed

Solution

Heat absorbed by sign's glass can be formulated :

$\tt Q=m.c.\Delta T$

ΔT=65.5 - 23.5 = 42

$\tt Q=905\times 0.67\times 42\\\\Q=\boxed{\bold{25466.7~J}}$

5 0

3 years ago

Read 2 more answers

Gaseous butane, CH3(CH2)2CH, reacts with gaseous oxygen gas, O2, to produce gaseous carbon dioxide, CO2, and gaseous water, H2O.

weeeeeb [17]

Answer:

Percentage yield of carbon dioxide is 49.9%

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

2CH3(CH2)2CH3 + 13O2 —> 8CO2 + 10H2O

2C4H10 + 13O2 —> 8CO2 + 10H2O

Next, we shall determine the masses of butane and oxygen that reacted and the mass of carbon dioxide produced from the balanced equation. This is illustrated below:

Molar mass of butane C4H10 = (12×4) + (10×1)

= 48 + 10

= 58 g/mol

Mass of C4H10 from the balanced equation = 2 × 58 = 116 g

Molar mass of O2 = 16 × 2 = 32 g/mol

Mass of O2 from the balanced equation = 13 × 32 = 416 g

Molar mass of CO2 = 12 + (16×2)

= 12 + 32

= 44 g/mol

Mass of CO2 from the balanced equation = 8 × 44 = 352 g

Summary:

From the balanced equation above,

116 g of butane reacted with 416 g of oxygen to produce 352 g of carbon dioxide.

Next, we shall determine the limiting reactant. This can be obtained as follow:

From the balanced equation above,

116 g of butane reacted with 416 g of oxygen.

Therefore, 34.29 g of butane will react with = (34.29 × 416) / 116 = 122.97 g of oxygen.

From the calculation made above, we can see clearly that only 122.97 g out of 165.7 g of oxygen reacted completely with 34.29 g of butane. Therefore, butane is the limiting reactant and oxygen is the excess reactant.

Next, we shall determine the theoretical yield of carbon dioxide.

In this case, we shall use the limiting reactant because it will give the maximum yield of carbon dioxide as all of it is used up in the reaction.

The limiting reactant is butane and the theoretical yield of carbon dioxide can be obtained as follow:

From the balanced equation above,

116 g of butane reacted to produce 352 g of carbon dioxide.

Therefore, 34.29 g of butane will react to produce = (34.29 × 352) / 116 = 104.05 g of carbon dioxide.

Therefore, the theoretical yield of carbon dioxide is 104.05 g

Finally, we shall determine the percentage yield of carbon dioxide as follow:

Actual yield of carbon dioxide = 51.9 g

Theoretical yield of carbon dioxide = 104.05 g

Percentage yield of carbon dioxide =?

Percentage yield = Actual yield /Theoretical yield × 100

Percentage yield of carbon dioxide = 51.9 / 104.05 × 100

Percentage yield of carbon dioxide = 49.9%

7 0

3 years ago

Thre largest source of available freshwater on earth is

Burka [1]

Ice caps so it would be D

Hope it helps :-)

6 0

3 years ago

Read 2 more answers