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Burka [1]
3 years ago
15

A gas has a pressure of 1.34 atm when the temperature is 237K. The gas is then heated until the temperature measures 312K. What

will be the new pressure?
Chemistry
1 answer:
alexandr1967 [171]3 years ago
6 0

The answer for the following question is answered below.

  • <em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>

Explanation:

Given:

Initial pressure of the gas = 1.34 atm

Initial temperature of the gas = 273 K

final temperature of the gas = 312 K

To solve:

Final temperature of the gas

We know;

From the ideal gas equation

P × V = n × R × T

So;

from the above equation we can say that

    <em>P ∝ T</em>

     \frac{P}{T} = constant  

     \frac{P_{1} }{P_{2} } = \frac{T_{1} }{T_{2} }

Where;

P_{1} = initial pressure of a gas

P_{2} = final pressure of a gas

T_{1} = initial temperature of a gas

T_{2} = final temperature of  a gas

    P_{2} = \frac{1.34*312}{237}

    P_{2}  = 1.76 atm

<em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>

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A chemist determined by measurements that 0.050 moles of aluminum participated in a chemical reaction. Calculate the mass of alu
Law Incorporation [45]

Answer:

13.5 g

Explanation:

This question is solved easily if we remember that the number of moles is obtained by dividing the mass into the atomic weight or molar mass depending if we are referring to elements or molecules.

Therefore, the mass of aluminum in the reaction will the 0.050 mol Al times the atomic weight of aluminum.

number of moles = n = mass of Al / Atomic Weight Al

⇒ mass Al = n x Atomic Weight Al = 0.050 mol x 27 g mol⁻¹

                                                         = 13.5 g

We have three significant figures in 0.050 and therefore we should have three significant figures in our answer.

           

8 0
3 years ago
I need help please j
Sidana [21]
Reactants Hydrogen: 5
Products Hydrogen: 5

Reactants Carbon: 3
Products Carbon: 3

Reactants Oxygen: 4
Products Oxygen: 5
3 0
3 years ago
Identify the gas law that applies to the following scenario: If a gas in a closed container is pressurized from 18.0 atm to 14.0
nalin [4]

Answer:

Gay-Lussac's Law

Explanation:

The pressure is directly proportional to the absolute temperature under constant volume. This states the Gay-Lussac's law. The equation is:

P1T2 = P2T1

<em>Where P is pressure and T absolute temperature of 1, initial state and 2, final state of the gas.</em>

<em />

That means the right option is:

- Gay-Lussac's Law

6 0
2 years ago
Temperature also affects the motion of atoms in a gas. Given what you know about temperature, pressure, and volume, which statem
vampirchik [111]

Answer:

C) As a gas is heated, the pressure decreases.

Explanation:

From the choices given, the statement that "as a gas is heated, the pressure decreases is false".

When gases are heated, their molecules expands and the volume of the gas increases. In a fixed container, the pressure of the gases will also increases.

  • Gases lack internal cohesion and very weak to no intermolecular forces binding them together.
  • When they are subjected to heat, they gain more energy(kinetic energy) which causes them to begin to spread out.
  • Thus, they take up even more space allowing volume to increase appreciably.

3 0
3 years ago
How many moles of oxygen gas are there in 395 L of oxygen at STP?
kozerog [31]

Answer:

17.6 moles of oxygen gas.

Explanation:

STP Variables:

P=1 atm

R=0.082

T=273 K

Use the PV=nRT, then plug in.

n=PV/RT

n= (1 atm)(395 L)/(0.082) (273 K)

Simplify.

n=17.6 moles of O2

Hoped this helped.

7 0
2 years ago
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