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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

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Which of the following is a balanced equation? Select one: a. A b. B c. C d. D

Phantasy [73]

Answer:

Explanation:

Balanced equations have the same number of elements on both sides. If the number of elements are equal to each other for every element in the equation on both sides, then the equation is balanced.

Important concept : The big number before an element or compound represents how many molecules of that compound or element there are in a reaction. To find the number of atoms of each element you multiply the coefficient by the subscript ( small number ) which represents the number of atoms of that element in each molecule. Ex. 3H2O. There is a coefficient of 3 meaning that there are 3 molecules of H2O. There is a subscript after H meaning there are 2 atoms of hydrogen in each molecule. To find the total number of atoms we multiply the subscript of hydrogen by the coefficient of the whole molecule. 3 * 2 = 6 , so there are a total of 6 atoms of hydrogen in 3H2O

A) Cu + 2AgNO3 ==> CuNO3 + 2Ag

1 Cu 1

2 Ag 2

2 N 1

3 O 3

The amount of nitrogen atoms is different on both sides of the equation therefore this is not a balanced equation

B) CCl4 + O2 ==> CO2 + 2Cl2

1 C 1

4 Cl 4

2 O 2

The number of atoms of each element is the same on both sides of the equation therefore this is the balanced equation, however lets check the other answer choices just in case.

C) 2K + H2SO4 ==> K2SO4 + 2H2

2 K 2

1 H 4

1 S 1

4 O 4

The number of Hydrogen atoms are different on each side of the equation therefore this is not a balanced equation.

D) 2Al2O3 ==> 2Al + 3O2

4 Al 2

6 O 6
There are a different amount of aluminum atoms on both sides of the equation therefore this is not a balanced equation.

3 0

2 years ago

S(s)+3F2(g)->SF6(g) how many mol of F2 are required to react completely with 2.30 mol of S?

Brilliant_brown [7]

Answer: There are 6.9 mol of $F_{2}$ are required to react completely with 2.30 mol of S.

Explanation:

The given reaction equation is as follows.

$S(s) + 3F_{2}(g) \rightarrow SF_{6}(g)$

Here, 1 mole of S is reaction with 3 moles of $F_{2}$ which means 1 mole of S requires 3 moles of $F_{2}$ .

Therefore, moles of $F_{2}$ required to react completely with 2.30 moles S are calculated as follows.

$1 mol S = 3 mol F_{2}\\2.30 mol S = 3 mol F_{2} \times 2.30 \\= 6.9 mol F_{2}$

Thus, we can conclude that there are 6.9 mol of $F_{2}$ are required to react completely with 2.30 mol of S.

3 0

3 years ago

How many moles of helium is required to blow up a balloon to 87.1 liters at 74 C and 3.5 atm?

marshall27 [118]

Moles of helium is required to blow up a balloon to 87.1 liters at 74 C and 3.5 atm is 021.65 mole

Mole is the unit of amount of substances of specified elementary entities

According to the ideal gas law he number of moles of a gas n can be calculated knowing the partial pressure of a gas p in a container with a volume V at an absolute temperature T from the equation

n =pV/RT

Here given data is volume = 87.1 liters

Temperature = 74 °C means 347.15 k

Pressure = 3.5 atm

R = 0.0821

Putting this value in ideal gas equation then

n =pV/RT

n = 3.5 atm×87.1 liters / 0.0821 ×347.15 k

n = 021.65 mole

Moles of helium is required to blow up a balloon to 87.1 liters at 74 C and 3.5 atm is 021.65 mole

Know more about mole of helium

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8 0

11 months ago

If 12.8 g of CaCO3 decomposes at 38 degrees C and 0.96 atm, how many dm3 of CO2 are formed in addition to CaO? CaCO3 → CaO + CO2

jasenka [17]

Answer:

3.4dm3

Explanation:

We'll begin by calculating the number of mole of CaCO3 present in 12.8g of CaCO3.

This can be achieved as shown below:

Molar Mass of CaCO3 = 40 + 12 + (16x3) = 40 + 12 + 48 = 100g/mol

Mass of CaCO3 obtained from the question = 12.8g

Number of mole of CaCO3 =?

Number of mole = Mass /Molar Mass

Number of mole of CaCO3 = 12.8/100

Number of mole of CaCO3 = 0.128 mole

The equation for the reaction is given below:

CaCO3 → CaO + CO2

From the equation above,

1 mole of CaCO3 produced 1 mole of CO2.

Therefore, 0.128 mole of CaCO3 will also produce 0.128 mole of CO2.

Now, we can obtain the volume of CO2 produced as follow:

Data obtained from the question include:

T (temperature) = 38°C = 38 + 273 = 311K

P (pressure) = 0.96 atm

n (number of mole of CO2) = 0.128 mole

R (gas constant) = 0.082atm.dm3/Kmol

V (volume of CO2) =?

Using the ideal gas equation PV = nRT, the volume of CO2 produced can be obtained as shown:

PV = nRT

0.96 x V = 0.128 x 0.082 x 311

Divide both side by 0.96

V = (0.128 x 0.082 x 311) /0.96

V = 3.4dm3

Therefore, 3.4dm3 of CO2 are produced.

7 0

3 years ago

Determine the net force acting on the object. Then, write whether or not there will be a change in motion. If yes, write the dir

quester [9]

Answer:

Net force= -5N+5N =0

Therefore there is no change in motion

Explanation:

3 0

2 years ago