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daser333 [38]
3 years ago
15

A gas occupies 900.0 ML at temperatures of 27.0 Celsius. What is the volume at 123.0 celsius

Chemistry
2 answers:
Artemon [7]3 years ago
4 0

Answer:

1188.0 mL.

Explanation:

  • We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.

  • If n and P are constant, and have two different values of V and T:

<em>V₁T₂ = V₂T₁ </em>

V₁ = 900 mL, T₁ = 27.0°C + 273 = 300.0 K.

V₂ = ??? mL, T₂ = 123.0°C + 273 = 396.0 K.

<em>∴ V₂ = V₁T₂/T₁ </em>= (900 mL)(396 K)/(300.0 K) = <em>1188.0 mL.</em>

Tamiku [17]3 years ago
3 0

Answer:

1188 ml

Explanation:

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When a substance is in the process of changing phases states of matter what happens to the temperature
Reptile [31]

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Temperature stays constant.

Explanation:

During a phase change, the temperature does not change. Temperature will only change when a phase change is completed.

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2 years ago
State with reasons, whether sulphur dioxide is acting as an oxidizing agent or a reducing agent in each of the following reactio
evablogger [386]

Answer:

A) oxidizing agent is SO2

B) NaClO is the oxidizing agent

Explanation:

A) This is a redox reaction in which oxidation and reduction occur simultaneously.

Thus, in 2H2S(g) + SO2(g) -> 2H2O(l) + 3S(s);

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H2S → S + 2H+ + 2e−

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4 0
3 years ago
*PLEASE HELP ASAP*
dimulka [17.4K]
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5 0
3 years ago
How much ice (in grams) would have to melt to lower the temperature of 353 mL of water from 26 ∘C to 6 ∘C? (Assume the density o
Rashid [163]

Answer:

The mass of ice required to melt to lower the temperature of 353 mL of water from 26 ⁰C to 6 ⁰C is 85.4197 kg

Explanation:

Heat gain by ice = Heat lost by water

Thus,  

Heat of fusion + m_{ice}\times C_{ice}\times (T_f-T_i)=-m_{water}\times C_{water}\times (T_f-T_i)

Where, negative sign signifies heat loss

Or,  

Heat of fusion + m_{ice}\times C_{ice}\times (T_f-T_i)=m_{water}\times C_{water}\times (T_i-T_f)

Heat of fusion = 334 J/g

Heat of fusion of ice with mass x = 334x J/g

For ice:

Mass = x g

Initial temperature = 0 °C

Final temperature = 6 °C

Specific heat of ice = 1.996 J/g°C

For water:

Volume = 353 mL

Density (\rho)=\frac{Mass(m)}{Volume(V)}

Density of water = 1.0 g/mL

So, mass of water = 353 g

Initial temperature = 26 °C

Final temperature = 6 °C

Specific heat of water = 4.186 J/g°C

So,  

334x+x\times 1.996\times (6-0)=353\times 4.186\times (26-6)

334x+x\times 11.976=29553.16

345.976x = 29553.16

x = 85.4197 kg

Thus,  

<u>The mass of ice required to melt to lower the temperature of 353 mL of water from 26 ⁰C to 6 ⁰C is 85.4197 kg</u>

7 0
3 years ago
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