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3 years ago

Which equation is set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22°C and 100 kPa?

Chemistry

1 answer:

LenKa [72]3 years ago

6 0

The volume could be calculated by using V = n RT / P 

In which V = Volume
n = number of Moles
R= The Gas constant
T = Temperature (ideally this would be in Kelvin, but i don't see it in the option)
P = Pressure

I believe the answer is

V = (1.5mol) (0.08205 L*kPa/K*mol) (22Celsius)/100 kPa

You might be interested in

What is the value of the van't Hoff factor for KCl if a 1.00m aqueous solution shows a vapor pressure depression of 0.734 mmHg a

yaroslaw [1]

Answer: The Van't Hoff factor for KCl is 1.74

Explanation:

We are given:

Molality of solution = 1 m

This means that 1 mole of a solute is present in 1 kg of solvent (water) or 1000 grams of water

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of water = 1000 g

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

$\text{Moles of water}=\frac{1000g}{18g/mol}=55.56mol$

Mole fraction of a substance is given by:

$\chi_A=\frac{n_A}{n_A+n_B}$

Moles of solute = 1 moles

Total moles = [1 + 55.56] = 56.56 moles

Putting values in above equation, we get:

$\chi_{(solute)}=\frac{1}{56.56}=0.0177$

The equation used to calculate relative lowering of vapor pressure follows:

$\frac{p^o-p_s}{p^o}=i\times \chi_{solute}$

where,

$\frac{p^o-p_s}{p^o}$ = relative lowering in vapor pressure = 0.734 mmHg

i = Van't Hoff factor = ?

$\chi_{solute}$ = mole fraction of solute = 0.0177

$p^o$ = vapor pressure of pure water = 23.76 torr

Putting values in above equation, we get:

$\frac{0.734}{23.76}=i\times 0.0177\\\\i=1.74$

Hence, the Van't Hoff factor for KCl is 1.74

7 0

3 years ago

PLEASE HELP ME ASAP!!!! PLEASE!!!!!!!!!! I will give brainliest and 20 points!! PLEASE!

Vika [28.1K]

#1
The rate of diffusion of a gas is inversely proportional to the square root of its molecular weight.
#2
shape, molecular weight. I don't know for sure though
#3
O2, N2, Ar, H2O vapor

5 0

3 years ago

What mass of sulfur has to burn to produce 4.5l so2 at 300°c and 101kpa s(s) o2( g. so2( g.?

Mandarinka [93]

S + O2 --> So2. P = 101kPa = 1atm. R = 0.082 atm - L - (mol-K)^-1. Applying ideal gas equation PV = nRT. n = 1x4.5/0.082x573 = 0.096mole. According to stoichiometry, moles of S = moles of SO2 = 0.096mol. Mass of S = moles of So2 x molar Wt = 0.095x32 = 3.04moles. Hope it helps

8 0

3 years ago

if the energy in a serving of food can heat up 450,000 grams of water 1°C, how many Calories are in the serving?

ahrayia [7]

I don’t know?I think but I’m not sure

3 0

3 years ago

Consider the following three samples. A. A sample containing 180 g glucose (C6H12O6) B. A sample containing 90 g glucose and 90

Aloiza [94]

Answer:

E) All three samples have the same number of hydrogen atoms

Explanation:

The statements are:

A) Sample A has more hydrogen atoms than sample B or sample C.

B) Sample B has more hydrogen atoms than sample A or sample C.

C) Sample C has more hydrogen atoms than sample A or sample B

D) Both samples A and C have the same number of hydrogen atoms, but more than in sample B.

E) All three samples have the same number of hydrogen atoms

Hydrogens in sample A are:

180g × (1mol Glucose / 180.156g) × (12mol H / 1 mol Glucose) = 12 moles of H

Hydrogens in sample B are:

90g Glucose × (1mol Glucose / 180.156g) × (12mol H / 1 mol Glucose) = 6 moles of H

90g mannose× (1mol Mannose / 180.156g) × (12mol H / 1 mol Glucose) = 6 moles of H

Total moles: 12

Hydrogens in sample C are:

180g × (1mol Mannose / 180.156g) × (12mol H / 1 mol Glucose) = 12 moles of H

Thus, right answer is:

E) All three samples have the same number of hydrogen atoms

I hope it helps!

8 0

3 years ago