A 100 kg block of wood was nearly cut into two smaller pieces what is the total mass of all the smaller pieces put together

Calculate the density of chloroform

Rina8888 [55]

Answer: The density of chloroform is 1.47 g/mL

Explanation : Given,

Volume = 40.5 mL

Mass of cylinder = 85.16 g

Mass of cylinder and liquid = 145.10 g

First we have to calculate the mass of liquid (chloroform).

Mass of liquid = Mass of cylinder and liquid - Mass of cylinder

Mass of liquid = 145.10 g - 85.6 g

Mass of liquid = 59.5 g

Now we have to calculate the density of liquid (chloroform).

Formula used:

$Density=\frac{Mass}{Volume}$

Now putting g all the given values in this formula, we get:

$Density=\frac{59.5g}{40.5mL}$

$Density=1.47g/mL$

Therefore, the density of chloroform is 1.47 g/mL

5 0

3 years ago

Which substance can not be broken down by a chemical change? silicon propane ethane water

babunello [35]

I think the answer is silicon :))

5 0

3 years ago

Read 2 more answers

As illustrated, the below manometer consists of a gas vessel and an open-ended U-tube containing a nonvolatile liquid with a den

STALIN [3.7K]

Answer:

1.01atm is the pressure of the gas

Explanation:

The difference in heights in the two sides is because of the difference in pressure of the enclosed gas and the atmospheric pressure. This difference is in mm of the nonvolatile liquid. The difference in mm Hg is:

32.3mm * (0.993g/mL / 13.6g/mL) = 2.36mmHg

As atmospheric pressure is 765mm Hg and assuming the gas has more pressure than the atmospheric pressure (There is no illustration), the pressure of the gas is:

765mm Hg + 2.36mm Hg = 767.36 mmHg

In atm:

767.36 mmHg * (1atm / 760 mmHg) =

1.01atm is the pressure of the gas

5 0

3 years ago

What is the temperature of 1.2 moles of helium gas at 2.57 ATM if it occupies 15.5L of volume

agasfer [191]

We will assume helium to behave as an ideal gas and apply the ideal gas law:
PV = nRT
For pressure measured in atmospheres and volume measured in liters, the value of the molar gas constant is 0.082. Therefore:
T = PV / nR
T = (2.57 x 15.5) / (1.2 x 0.082)
T = 404.8 Kelvin

8 0

3 years ago

How many atoms of sulfur, S, are in 4.00 g sulfur?

Angelina_Jolie [31]

<h3>Answer:</h3>

7.51 × 10²² atoms S

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

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Table
Using Dimensional Analysis
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<h3>Explanation:</h3>

<u>Step 1: Define</u>

4.00 g S

<u>Step 2: Identify Conversions</u>

Avogadro's Number

Molar Mass of S - 32.07 g/mol

<u>Step 3: Convert</u>

Set up: $\displaystyle 4.00 \ g \ S(\frac{1 \ mol \ S}{32.07 \ g \ S})(\frac{6.022 \cdot 10^{23} \ atoms \ S}{1 \ mol \ S})$
Multiply: $\displaystyle 7.51107 \cdot 10^{22} \ atoms \ S$

<u>Step 4: Check</u>

<em>Follow sig figs and round. We are given 3 sig figs.</em>

7.51107 × 10²² atoms S ≈ 7.51 × 10²² atoms S

5 0

3 years ago