Greatest<br> –9.2 x 10-2<br> -8.9 x 102<br> --4.39 x 10-5<br> -2.182, 100<br> Least

At what temperature does uranium hexafluoride have a density of 0.5820 g/L at 0.5073 atm?

Svet_ta [14]

Answer:

4204 K

Explanation:

Step 1: Data

<em>Given data</em>

Density of uranium hexafluoride (ρ): 0.5820 g/L

Pressure of uranium hexafluoride (P): 0.5073 atm

<em>Required data</em>

Universal gas constant (R): 0.08206 atm.L/mol.K

Molar mass of uranium hexafluoride (M): 352.02 g/mol

Step 2: Calculate the temperature of the gas

We will use the following expression derived from the ideal gas equation.

P × M = ρ × R × T

T = P × M/ρ × R

T = 0.5073 atm × (352.02 g/mol)/(0.5820 g/L) × (0.08206 atm.L/mol.K)

T = 4204 K

8 0

3 years ago

Difference between fission and fusion?

algol13

The difference is the following: Fission is when a heavy nucleus is very unstable and is splitted into two lighter nuclei. Fusion is in a sense the contrary process: two light nuclei combine and release more energy

4 0

3 years ago

When a 3.80 g sample of magnesium nitride (MW 101g/mol) is reacted with 3.30 g of water, 3.60 g of MgO is formed. What is the pe

lianna [129]

The percent yield of this reaction is calculated as follows
Mg3N2 + 3H2O =2NH3 + 3Mgo

calculate the theoretical yield,
moles=mass/molar mass
moles Mg3N2= 3.82 g/100g/mol= 0.0382 moles(limiting regent)

moles of H2o= 7.73g/18g/mol = 0.429 moles ( in excess_)

by use of mole ratio between Mg3N2 to MgO which is 1:3 the moles of MgO = 0.0382 x3 = 0.1146 moles
mass =moles x molar mass

the theoretical mass is therefore = 0.1146mole x 40 g/mol = 4.58 grams

The % yield = actual mass/theoretical mass x1000

= 3.60/4.584 x100= 78.5%

3 0

3 years ago

Read 2 more answers

How much of a 1.00 mg sample of americium remains after 3 half-lives?

notka56 [123]

Answer: 0.125mg americium

Half-lives is a set of duration when a sample will become half of their original mass. In this case, the initial mass is 1mg and the sample is going for 3 times half-lives. Then the calculation would be: 1mg $1/2^{3}$ = 1/8 mg= 0.125mg.

5 0

3 years ago

Read 2 more answers

The main constituent of gallstones is cholesterol. Cholesterol may have a role in heart attacks and blood clot formation. Its el

Nataly [62]

The main constituent of gallstones is cholesterol. Cholesterol may have a role in heart attacks and blood clot formation. Its elemental percentage composition is 83.87% C, 11.99% H, and 4.14% O. It has a molecular weight of 386.64 amu. Empirical formula is C₃H₄O₁ and Molecular formula is 7(C₃H₄O₁).

<h3>What is Empirical Formula ?</h3>

Empirical formula is the simplest whole number ratio of atoms present in given compound.

Element % Atomic mass Relative no. of atoms Simplest whole ratio

C 83.87 12 $\frac{83.87}{12}$ = 6.98 $\frac{6.98}{0.25}$ = 3

H 11.99 1 $\frac{11.99}{1}$ = 11.09 $\frac{11.09}{0.25}$ = 4

O 4.14 16 $\frac{4.14}{16}$ = 0.25 $\frac{0.25}{0.25}$ = 1

Thus the empirical formula is C₃H₄O₁.

<h3>How to find the Molecular formula of compound ?</h3>

Molecular formula = Empirical formula × n

n = $\frac{\text{Molecular weight}}{\text{Empirical formula weight}}$

= $\frac{386.64}{56}$

= 7

Molecular formula = Empirical formula × n

= 7 (C₃H₄O₁)

Thus from the above conclusion we can say that The main constituent of gallstones is cholesterol. Cholesterol may have a role in heart attacks and blood clot formation. Its elemental percentage composition is 83.87% C, 11.99% H, and 4.14% O. It has a molecular weight of 386.64 amu. Empirical formula is C₃H₄O₁ and Molecular formula is 7(C₃H₄O₁).

Learn more about the Empirical Formula here: brainly.com/question/1603500

#SPJ4

7 0

2 years ago

Greatest –9.2 x 10-2 -8.9 x 102 --4.39 x 10-5 -2.182, 100 Least