The principle of the wet-bulb thermometers states that __________

1. Which feature would most LIKELY be forming at converging continental tectonic plate

Simora [160]

I believe the answer would be a.

4 0

3 years ago

Methanol has a normal boiling point of 64.6C and a heat of vaporization of 35.2 kJ/mol. What is the vapor pressure (in Torr) of

DENIUS [597]

Answer:

vapor pressure of methanol at 12.0C = 75.09 torr

Explanation:

Using Clausius Clapeyron equation

, we have that

ln (P2/P1)= (ΔHvap /R) (1/T1 - 1/T2)

Given

At Normal boiling point,

Temperature T1= 64.6°C = 64.6 + 273 = 337.6 K, Pressure,P1 = 1 atm

Heat of vaporization = 35.2 kJ/mol

Changing to J/mol

=35.2 x 1000= 35200 J/mol

Temperature , T2 = 12.0oC = 12 + 273 = 285 K

Using gas constant, R = 8.314 J/mol.K

ln (P2/P1)= -(ΔHvap /R) (1/T1 - 1/T2)

ln (P2/ 1 atm) = (35200 J/mol/ (8.314 J/mol.K) X( 1/337.6 - 1/285)

ln (P2/ 1 atm) =4,233.822 X (0.00296-0.003508)

ln (P2/ 1 atm) = 4,233.822468 x-0.0005466866

ln (P2/ 1 atm)= -2.31457

P2 = e^⁻2.31457 x 1 atm

P2=0.098808atm

= 0.098808atm x760 = 75.09 torr

7 0

3 years ago

Propane burns in air to produce carbon dioxide and water?

Elan Coil [88]

Hey there!
Great question=)

Yes, this statement is true! Propane burns in air and it produces carbon dioxide and water.

I hope this helps;)

6 0

3 years ago

What volume did a helium-filled balloon have at 22.5 c and 1.95 atm if it’s new volume was 56.4 mL at 3.69 atm and 11.9c

Veseljchak [2.6K]

This is an exercise in the general or combined gas law.

To start solving this exercise, we obtain the following data:

T₁ = 22.5 °C + 273 = 295.5 K
P₁ = 1.95 atm
V₁ = ¿?
P₂ = 3.69 atm
T₂ = 11.9 °C + 273 = 284.9 k
V₂= 56.4 ml

We use the following formula:

P₁V₁T₂ = P₂V₂T₁ ⇒ General formula

Where

P₁ = Initial pressure
V₁ = Initial volume
T₂ = Initial temperature
P₂ = Final pressure
V₂ = final volume
T₁ = Initial temperature

We clear the formula for the initial volume:

$\boldsymbol{\sf{V_{1}=\dfrac{P_{2}V_{2}T_{1}}{P_{1}T_{2}} } }$

We substitute our data into the formula to solve:

$\boldsymbol{\sf{V_{1}=\dfrac{(3.69 \not{atm})(56.4 \ ml)(295.5 \not{k})}{(1.95 \not{atm})(284.9\not{k})} }}$

$\boldsymbol{\sf{V_{1}=\dfrac{61498.278}{555.555} \ lm }}$

$\boxed{\boldsymbol{\sf{V_{1}=110.697 \ lm }}}$

The helium-filled balloon has a volume of <u>110.697 ml.</u>

6 0

1 year ago

Read 2 more answers

Citric acid is often used as an acidity regulator in hot water canning of tomatoes. At 25°C it has Kat 7.4x10- and A.Hº = +4.1 k

gavmur [86]

Answer:

The rate constant at T = 100 C is 1.0*10⁻³

Explanation:

The Arrhenius equation relates two rate constants K1 and K2 measured at temperatures T1 and T2 as shown below:

$ln\frac{K_{2}}{K_{1}}=\frac{\Delta H^{0}rxn}{R}(\frac{1}{T_{1}}-\frac{1}{T_{2}})$

here, ΔHrxn = standard enthalpy change of the reaction

R = gas constant

From the given information:

K1 = 7.4*10^-4

T1 = 25 C = 25+273 = 298 K

T2 = 100 C = 100+273 = 373K

ΔH°=4.1kJ/mol

$ln\frac{K_{2}}{7.4*10^{-4}}=\frac{4.1 kJ/mol}{0.08314kJ/mol.K}(\frac{1}{298}-\frac{1}{373})K$

K2 = 1.03*10⁻³

6 0

3 years ago

The principle of the wet-bulb thermometers states that ___________.