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anyanavicka [17]
2 years ago
7

The absolute temperature of a gas is increased four times while maintaining a constant volume. What happens to the

Chemistry
1 answer:
weqwewe [10]2 years ago
4 0

Answer:

The pressure increases by a factor of four.

Explanation:

Let's consider a gas at a given temperature and pressure (T₁, P₁). The absolute temperature of a gas is increased four times (T₂ = 4 T₁) while maintaining a constant volume. We can assess the effect on the pressure (P₂) by using Gay Lussac's law.

P₁/T₁ = P₂/T₂

P₂ = P₁ × T₂/T₁

P₂ = P₁ × 4 T₁/T₁

P₂ = 4 P₁

The pressure increases by a factor of four.

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erastovalidia [21]

Answer:

Re=309926.13

Explanation:

density=92.8lbm/ft3*(0.45kg/1lbm)*(1ft3/0.028m3)=1491.43kg/m3

viscosity=4.1cP*((1*10-3kg/m*s)/1cP)=0.0041kg/m*s

velocity=237ft/min*(1min/60s)*(0.3048m/1ft)=1.2m/s

diameter=28inch*(0.0254m/1inch)=0.71m

Re=(density*velocity*diameter)/viscosity=(1491.43kg/m3*1.2m/s*0.71m)/0.0041kg/m*s

Re=309926.13

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3 years ago
How many moles of sulfur will be needed to oxidize 3 moles of zinc to zinc sulfide
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Aobt 1,200 halp you at all
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3 years ago
What is the formula for tricarbon heptafluoride?<br> C2F3<br> CF7<br> C3F7<br> C773
bagirrra123 [75]

Answer:

C3F7

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hence F7

3 0
2 years ago
Please help ASAP. No one could not help me with this question.
Tanya [424]

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3 0
2 years ago
A hot air balloon is filled with 15 moles helium gas and 5 moles nitrogen gas. What is the volume of the balloon at 1.01 atm and
kvasek [131]

<u>Given:</u>

Moles of He = 15

Moles of N2 = 5

Pressure (P) = 1.01 atm

Temperature (T) = 300 K

<u>To determine:</u>

The volume (V) of the balloon

<u>Explanation:</u>

From the ideal gas law:

PV = nRT

where P = pressure of the gas

V = volume

n = number of moles of the gas

T = temperature

R = gas constant = 0.0821 L-atm/mol-K

In this case we have:-

n(total) = 15 + 5 = 20 moles

P = 1.01 atm and T = 300K

V = nRT/P = 20 moles * 0.0821 L-atm/mol-K * 300 K/1.01 atm = 487.7 L

Ans: Volume of the balloon is around 488 L


3 0
3 years ago
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