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2 years ago

At 25.5 °C and a pressure of 116.1 kPa a sample of gas has a volume of

Chemistry

1 answer:

Darina [25.2K]2 years ago

4 0

Answer:

64 ahmx loumming (486.4 mmHg! 8 kpa. ODEIO! d.) 3140mmiga 7 commotty. 4. TEMPERATURE ... A gas has a volume of 300 mL at 300 mm Hg. What will its volume be if the pressure is changed to 500.

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Write the symbols of following elements. a. Phosphorus b. Bromine c. Silver d. Sodium

Vikki [24]

Answer:

a. P

b. Br

c. Ag

d. Na

Explanation:

The Periodic Table says so

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2 years ago

Which statement is true about a pseudoscientific idea? It is biased in its results. It can be tested and observed. It can be rep

vesna_86 [32]

<span>It is biased in its results.

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6 0

3 years ago

Read 2 more answers

A hot air balloon is filled with 1.31 × 10 6 L of an ideal gas on a cool morning ( 11 ∘ C ) . The air is heated to 121 ∘ C . Wha

victus00 [196]

Answer:

$1.82\times 10^6 L$ is the volume of the air in the balloon after it is heated.

Explanation:

To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$ (at constant pressure)

where,

$V_1\text{ and }T_1$ are the initial volume and temperature of the gas.

$V_2\text{ and }T_2$ are the final volume and temperature of the gas.

We are given:

$V_1= 1.31\times 10^6 L\\T_1=11^oC=(11+273.15)K=284.15K\\V_2=?\\T_2=121^oC=(121+273.15)K=394.15 K$

Putting values in above equation, we get:

$\frac{1.31\times 10^6 L}{284.15 K}=\frac{V_2}{394.14 K}\\\\V_2=\frac{V_1\times T_2}{T_1}$

$V_2=1.82\times 10^6 L$

$1.82\times 10^6 L$ is the volume of the air in the balloon after it is heated.

4 0

3 years ago

(reply if you know the answer or get reported) How many atoms are there in 5 grams of silicon?

joja [24]

Similarly, for one gram atomic weight of silicon with atomic weight of 28 grams, one mole of silicon still contains 6.022 × 1023 silicon atoms.Answer:

Explanation:

hope it helps

4 0

2 years ago

What pressure is exerted by 0.750 mol of a gas at 0 °C and a volume of 5

kow [346]

Answer: 3.4 atm

Explanation:

Given that:

Volume of gas V = 5L

(since 1 liter = 1dm3

5L = 5dm3)

Temperature T = 0°C

Convert Celsius to Kelvin

(0°C + 273 = 273K)

Pressure P = ?

Number of moles of gas n = 0.75 moles

Note that Molar gas constant R is a constant with a value of 0.0821 atm dm3 K-1 mol-1

Then, apply ideal gas equation

pV = nRT

p x 5dm3 = 0.75 moles x (0.0821 atm dm3 K-1 mol-1 x 273K)

p x 5dm3 = 16.8 atm dm3

p = (16.8 atm dm3 / 5dm3)

p = 3.4 atm

Thus, a pressure of 3.4 atm is exerted by the gas.

7 0

3 years ago