Suppose that the volume of a particular sample of cl2 is 718 ml at 675 mmhg and 48c at what temperature in c will the volume be 2.0 l if the pressure is 159 kpa

1900 °C

Step-by-step explanation:

This looks like a case where we can use the Combined Gas Law to calculate the temperature.

p₁V₁/T₁ = p₂V₂/T₂               Multiply both sides by T₂

p₁V₁T₂/T₁ = p₂V₂                 Multiply each side by T₁

p₁V₁T₂ = p₂V₂T₁                   Divide each side by p₁V₁

T₂ = T₁ × p₂/p₁ × V₂/V₁  

Data:

We must convert the pressures to a common unit. I have chosen atmospheres.

p₁ = 675 mmHg × 1atm/760 mmHg = 0.8882 atm

V₁ = 718 mL = 0.718 L

T₁ = 48 °C = 321.15 K

p₂ = 159 kPa × 1 atm/101.325 kPa = 1.569 atm

V₂ = 2.0 L

T₂ = ?

Calculation:

T₂ = 321.15 × 1.569/0.8882 × 2.0/0.718  

T₂ = 321.15 × 1.766 × 2.786  

T₂ = 321.15 × 1.569/0.8882 × 7.786  

T₂ = 1580K  

T₂ = 1580 + 273.15

T₂ = 1900 °C

Note: The answer can have only two significant figures because that is all you gave for the second volume of the gas.

it is a good conductor

explanation:

i'm wiling to try and you : )