All categories

3 years ago

HELP WILL GIVE BRAINLIEST!!

Chemistry

1 answer:

prohojiy [21]3 years ago

4 0

Answer:

This if from lowest to highest

Parked truck
Slow car (depending on its actual speed)
Fast feather (depending on how its falling)
Fast baseball
Fast car (depends on it's mph)

You might be interested in

Will Mark Brainly if correct.

lidiya [134]

The question is not clear
sorry

4 0

3 years ago

Given: 36.7 grams of CaF2 is added to 300 mL water. Find molarity?

BigorU [14]

<h3>Answer:</h3>

2 M

<h3>General Formulas and Concepts:</h3>

Math

Pre-Algebra

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right

Chemistry

Unit 0

Reading a Periodic Table
Using Dimensional Analysis

Aqueous Solutions

Molarity = moles of solute / liters of solution

<h3>Explanation:</h3>

Step 1: Define

36.7 g CaF₂

300 mL H₂O

Step 2: Identify Conversions

Molar Mass of Ca - 40.08 g/mol

Molar Mass of F - 19.00 g/mol

Molar Mass of CaF₂ - 40.08 + 2(19.00) = 78.08 g/mol

1000 mL = 1 L

Step 3: Convert

Solute

Set up: $\displaystyle 36.7 \ g \ CaF_2(\frac{1 \ mol \ CaF_2}{78.08 \ g \ CaF_2})$
Multiply: $\displaystyle 0.470031 \ mol \ CaF_2$

Solution

Set up: $\displaystyle 300 \ mL \ H_2O(\frac{1 \ L \ H_2O}{1000 \ mL \ H_2O})$
Multiply: $\displaystyle 0.3 \ L \ H_2O$

Step 4: Find Molarity

Substitute [M]: $\displaystyle x \ M = \frac{0.470031 \ mol \ CaF_2}{.3 \ L \ H_2O}$
Divide: $\displaystyle x = 1.56677 \ M$

Step 5: Check

Follow sig fig rules and round. We are given 1 sig fig as our lowest.

1.56677 M ≈ 2 M

8 0

3 years ago

What is the mass of 6.02 x 1022 atoms of Xenon? HELP!!!!!

il63 [147K]

So 6.02*10^22 is avogadro constant, which is the amount of atoms in one mole. If you look Xenon up in the periodic table you will find it's mass given 131,293, which is grams per 1 mole.

8 0

3 years ago

How do you know if a reaction is endothermic?

Bess [88]

If the temperature becomes colder

6 0

3 years ago

Read 2 more answers

How many liters of Cl2 gas will you have if you are using 63 g of Na?

ELEN [110]

Answer:

You will have 19.9L of Cl2

Explanation:

We can solve this question using:

PV = nRT; V = nRT/P

Where V is the volume of the gas

n the moles of Cl2

R is gas constant = 0.082atmL/molK

T is 273.15K assuming STP conditions

P is 1atm at STP

The moles of 63g of Cl2 gas are -molar mass: 70.906g/mol:

63g * (1mol / 70.906g) = 0.8885 moles

Replacing:

V = 0.8885mol*0.082atmL/molK*273.15K/1atm

V = You will have 19.9L of Cl2

6 0

3 years ago