What would be the pressure of a gas, at 101.3 kPa, if the temperature is lowered

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

Kryger [21]

Answer:

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.

4 0

3 years ago

Carbon disulfide burns in oxygen to yield carbon dioxide and sulfur dioxide according to the following chemical equation. CS2(l)

Semmy [17]

Answer:

a) the limiting reactant is 02

b) There will remain 0.667 moles of CS2

c) There will be formed 0.333 moles oof CO2 and 0.667 moles of SO2

Explanation:

Step 1: Data given

Number of moles of CS2 = 1.00 mol

Number of moles of O2 = 1.00 mol

Molar mass of O2 = 32 g/mol

Molar mass of CS2 = 76.14 g/mol

Step 2: The balanced equation

CS2(l) + 3O2(g) → CO2(g) + 2SO2(g)

Step 3: Calculate the limiting reactant

For 1 mole of CS2 we need 3 moles of O2 to produce 1 mol of CO2 and 2 moles of SO2

O2 is the limiting reactant. It will completely be consumed.(1.00 mol).

CS2 is in excess. There will react 1.00/ 3 = 0.333 moles

There will remain 1.00 - 0.333 = 0.667 moles of CS2

Step 4: Calculate moles of CO2 and SO2

For 1 mole of CS2 we need 3 moles of O2 to produce 1 mol of CO2 and 2 moles of SO2

For 1.00 mol of O2 we have 1.00/3 = 0.333 moles CO2

For 1.00 mol of O2 we have 1.00 /(3/2) = 0.667 moles of SO2

8 0

3 years ago

In what order are chemical elements arranged on the periodic table?

Gala2k [10]

Answer:

an increasng atomic number/ increasing proton count

Explanation:

3 0

3 years ago

A 64.0 ml volume of 0.25 m hbr is titrated with 0.50 m koh. calculate the ph after addition of 32.0 ml of koh at 25 ∘c.

aleksley [76]

Hello!

The reaction between HBr and KOH is the following:

HBr+KOH→H₂O + KBr

To calculate the amount of HBr left after addition of KOH, you'll use the following equations:

$HBr_f=HBr_i-KOH=([HBr]*vHBr)-([KOH]*vKOH) \\ \\ HBr_f=(0,25M*0,64L)-(0,5M*0,32L)=0 mol HBr$

That means that after the addition of 32 mL of KOH, there is no HBr left in the solution and the pH should be neutral, close to 7.

Have a nice day!

3 0

3 years ago

What types of orbital overlap occur in cumulene? check all that apply. check all that apply. p/p overlap sp/sp2 overlap s/sp ove

egoroff_w [7]

Cumulene is an alkene hydrocarbon that has two or three double bonds. It is also known as allene. The simplest cumulene is butatriene. It is a rigid hydrocarbon due to the presence of double bonds.

Answer: The orbital that overlap are p/p overlap, s/sp2 overlap, sp/sp2 overlap and sp/sp orbital.

8 0

3 years ago

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