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icang [17]
3 years ago
15

Balloon A started with a volume of 1.76 L. The temperature of the room the balloon was in was 295 K. The balloon was heated to a

temperature of 253.15 K. What is the new volume?
Chemistry
1 answer:
valentina_108 [34]3 years ago
4 0

Answer:

V₂ = 1.5 L

Explanation:

Given data:

Initial volume of balloon = 1.76 L

Initial temperature = 295 K

Final temperature = 253.15 K

Final volume = ?

Solution:

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁  

V₂ = 1.76 L ×253.15 K / 295 K

V₂ = 445.54 L.K /295 K

V₂ = 1.5 L

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What is the pressure of a gas that began at 38 torr, and 500L and is changed to occupy a volume of 677 L?
qwelly [4]

Answer:

P₂ = 28.5 torr

Explanation:

Given data:

Initial pressure = 38 torr

Initial volume = 500 L

Final volume = 677 L

Final pressure = ?

Solution:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = Initial volume

P₂ = Final pressure

V₂ = Final volume

Now we will put the vales in formula.

P₁V₁ = P₂V₂

P₂ = P₁V₁ /V₂

P₂ = 38 torr × 500 L / 667 L

P₂ = 19000 torr. L / 667 L

P₂ = 28.5 torr

6 0
3 years ago
54.56 g of water at 80.4 oC is added to a calorimeter that contains 47.24 g of water at 40 oC. If the final temperature of the s
fomenos

Answer:

49.5J/°C

Explanation:

The hot water lost some energy that is gained for cold water and the calorimeter.

The equation is:

Q(Hot water) = Q(Cold water) + Q(Calorimeter)

<em>Where:</em>

Q(Hot water) = S*m*ΔT = 4.184J/g°C*54.56g*(80.4°C-59.4°C) = 4794J

Q(Cold water) = S*m*ΔT = 4.184J/g°C*47.24g*(59.4°C-40°C) = 3834J

That means the heat gained by the calorimeter is

Q(Calorimeter) = 4794J - 3834J = 960J

The calorimeter constant is the heat gained per °C. The change in temperature of the calorimeter is:

59.4°C-40°C = 19.4°C

And calorimeter constant is:

960J/19.4°C =

<h3>49.5J/°C</h3>

<em />

7 0
2 years ago
What is the concentration in molarity of S2O32- (aq) in a solution prepared by mixing 150 mLmL of 0.149 MM Na2S2O3 (aq) with eno
Artist 52 [7]

Answer:

0.0890 M

Explanation:

Since the concentration of KCl is irrelevant in this case, the concentration of Na2S2O3 can be determined using a simple dilution equation:

C1V1 = C2V2, where C1 = 0.149 M, V1 = 150 mL, V2 = 250 mL

C2 = 0.149 x 150/250

                    = 0.089 M

To determine the concentration of  S2O32- (aq), consider the equation:

Na_2S_2O_3  => 2Na^+_{(aq)} + S_2O^2^-_3_{(aq)}

The concentration of Na2S2O3 and S2O32- (aq) is 1:1

Hence, the concentration in molarity of S2O32- (aq) is 0.089 M.

To 3 significant figures = 0.0890 M

7 0
2 years ago
How much does 1 gallon of water weigh in lbs? <br> Given: Density of water = 1 g/cm^3
saw5 [17]

Answer:

8.35 US lbs.

You don't need to know density for this problem... although it is another way to get the same solution.

5 0
2 years ago
If 0.034 moles of potassium nitrate were formed how many moles of lead (II) nitrate did you start
uranmaximum [27]

Answer:

0.017 mole of Pb(NO₃)₂.

Explanation:

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

2KOH + Pb(NO₃)₂ —> 2KNO₃ + Pb(OH)₂

From the balanced equation above,

1 mole of Pb(NO₃)₂ reacted to produce 2 moles of KNO₃.

Finally, we shall determine the number of mole of Pb(NO₃)₂ required to produce 0.034 mole of KNO₃. This can be obtained as follow:

From the balanced equation above,

1 mole of Pb(NO₃)₂ reacted to produce 2 moles of KNO₃.

Therefore, Xmol of Pb(NO₃)₂ will react to produce 0.034 mole of KNO₃ i.e

Xmol of Pb(NO₃)₂ = 0.034 / 2

Xmol of Pb(NO₃)₂ = 0.017 mole.

Thus, 0.017 mole of Pb(NO₃)₂ is needed for the reaction.

6 0
3 years ago
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