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2 years ago

How to find new pressure of gas if bottle explodes

1 answer:

6 0

If the container explodes there is no pressure, becuase all your gas has escaped its container, there for, you ain’t got no gas

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What are some non examples of temperature ?

Alja [10]

non examples of temperature are dixionanon , fairinheat, cabrowskin, and lastly ancomthere

6 0

2 years ago

Displacement vectors of 4km north, 2km south, 5km north, 5km south combine to a total displacement of

goldfiish [28.3K]

Answer

The combined displacement is 2km north

Explanation

Since displacement is a vector quantity, we take into account the direction.

Good for us all the displacement vectors are in the same dimension, so we can make north positive and south negative or vice-versa.

We now add to obtain,

$4+-2+5+-5$

This will simplify to

$=4-2+5-5=2$

Therefore the combined displacement is 2km north

5 0

2 years ago

A cylinder with a moving piston expands from an initial volume of 0.250 L against an external pressure of 2.00 atm. The expansio

Step2247 [10]

The final volume of the gas is 144.25 L

Explanation:

For an ideal gas kept at constant pressure, the work done by the gas on the surroundings is given by

$W=p\Delta V = p(V_f - V_i)$

where

p is the pressure of the gas

$V_i$ is the initial volume

$V_f$ is the final volume

For the gas in the cylinder in this problem,

p = 2.00 atm

$V_i = 0.250 L$

And we also know the work done,

W = 288 J

So we can solve the equation for $V_f$ , the final volume:

$V_f = V_i + \frac{W}{p}=0.250 + \frac{288}{2.00}=144.25 L$

Learn more about ideal gases:

brainly.com/question/9321544

brainly.com/question/7316997

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#LearnwithBrainly

7 0

2 years ago

We start with 5.00 moles of an ideal monatomic gas with an initial temperature of 128 ∘C. The gas expands and, in the process, a

o-na [289]

Answer:

The final temperature of the gas is 114.53°C.

Explanation:

Firstly, we calculate the change in internal energy, ΔU from the first law of thermodynamics:

ΔU=Q - W

ΔU = 1180 J - 2020 J = -840 J

Secondly, from the ideal gas law, we calculate the final temperature of the gas, using the change in internal energy:

$ΔU=\frac{3}{2} nRΔT$

$ΔU=\frac{3}{2} nR(T_{2} -T_{1} )$

Then we make the final temperature, T₂, subject of the formula:

$T_{2} =\frac{2ΔU}{3nR} +T_{1}$

$T_{2} =\frac{2(-840J)}{(3)(5)(8.314J/mol.K)} +128 deg.C$

$T_{2} =114.53 deg.C$

Therefore the final temperature of the gas, T₂, is 114.53°C.

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2 years ago

Students who embrace an innate mindset might view their poor performance in math as inevitable or beyond their control

PilotLPTM [1.2K]

Answer:

True

Explanation:

4 0

2 years ago

Read 2 more answers