All categories

3 years ago

What is the volume of 40.0 grams of argon gas at STP ?

Chemistry

1 answer:

MrRa [10]3 years ago

5 0

Answer:

24.9 L Ar

General Formulas and Concepts:

Atomic Structure

Reading a Periodic Table
Moles
STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K

Aqueous Solutions

States of Matter

Stoichiometry

Using Dimensional Analysis

Explanation:

Step 1: Define

[Given] 40.0 g Ar

[Solve] L Ar

Step 2: Identify Conversions

[PT] Molar Mass of Ar - 39.95 g/mol

[STP] 22.4 L = 1 mol

Step 3: Convert

[DA] Set up: $\displaystyle 40.0 \ g \ Ar(\frac{1 \ mol \ Ar}{39.95 \ g \ Ar})(\frac{22.4 \ L \ Ar}{1 \ mol \ Ar})$
[DA] Divide/Multiply [Cancel out units]: $\displaystyle 24.9235 \ L \ Ar$

Step 4: Check

Follow sig fig rules and round. We are given 3 sig figs.

24.9235 L Ar ≈ 24.9 L Ar

You might be interested in

Determine the number of carbon atoms in 1.00 kg of carbon dioxide.

olga2289 [7]

Answer:

1.37x10²⁵atoms of carbon

2.74x10²⁵ atoms of oxygen.

33.7g of KNO₃

Explanation:

To answer this question you must use molar mass of carbon dioxide (44g/mol) and 1 mole are 6.022x10²³atoms.

1.00kg are 1000g of CO₂. Moles are:

1000g CO₂ * (1mol / 44g) = 22.73 moles of CO₂ = 22.73 moles of carbon.

In atoms:

22.73 moles C * (6.022x10²³atoms / 1mole) = 1.37x10²⁵atoms of carbon

There are 22.73 moles of CO₂ * 2 = 45.45 moles of oxygen are present in the carbon dioxide. In atoms:

45.45 moles Oxygen * (6.022x10²³atoms / 1mole) = 2.74x10²⁵ atoms of oxygen.

1 mole of Potassium nitrate, KNO₃, contains 3 moles of oxygen. 1 mol of oxygen are:

1.00 mol O * (1mol KNO₃ / 3 moles O) = 0.33 moles of KNO₃

As molar mass of KNO₃ is 101.1g/mol:

0.33 moles of KNO₃ * (101.1g / mol) = 33.7g of KNO₃

5 0

3 years ago

Read 2 more answers

How many planets are in the solar system?

tatyana61 [14]

Eight PlanetsThere are eight planets in the solar system: Mercury, Venus, Earth, Mars, Jupiter, Saturn, Uranus, and Neptune.

But don't we wish for Pluto! :(

4 0

4 years ago

Read 2 more answers

Consider the following precipitation reaction (balanced). precipitation reaction: 2NH4Br(aq)+Pb(C2H3O2)2(aq)⟶2NH4C2H3O2(aq)+PbBr

sweet [91]

Answer:

Pb2+ (aq) & 2Br- (aq) --> PbBr2 (s).

Explanation:

Equation of the reaction:

Pb(C2H32O2)2 (aq) + 2 NH4Br (aq) --> 2NH4C2H3O2 (aq) + PbBr2 (s)

Ionic equation:

Pb+2(aq) + 2(C2H3O2)-1 (aq) + 2(NH4+) (aq) + 2Br-1 (aq) --> 2(NH4+) (aq) + 2(C2H3O2-) (aq) + PbBr2 (s)

2(NH4)+1(aq) & 2(C2H3O2)-1 (aq) cancel out from both sides, you are left with the net ionic equation :

Pb2+ (aq) & 2Br- (aq) --> PbBr2 (s).

6 0

3 years ago

What is the Kp of this reaction at 700oC if the Kc is 0.40?

dem82 [27]

I am pretty sure its D

3 0

3 years ago

Read 2 more answers

How much NaCl would you dissolve and dilute to the 100.00 mL mark in a volumetric flask with DI H2O to prepare a 0.825 M sodium

adoni [48]

Answer:

4.82 g

Explanation:

To solve this problem we'll use the definition of molarity:

Molarity = moles / liters

We are given the volume and concentration (keep in mind that 100mL=0.100L):

0.825 M = moles / 0.100 L

Now we calculate the number of NaCl moles required:

moles = 0.0825 mol

Then we convert 0.0825 NaCl moles into grams, using its molar mass:

0.0825 mol * 58.44 g/mol = 4.82 g

4 0

3 years ago