The density of copper is 8.9 g/ml. How many Cm of copper are in 0.283kg of copper?

Helllllllpppppppppppp<br><br>l

Ber [7]

Answer:

hi

Explanation:

6 0

3 years ago

3) Which of the following is a true statement

Hitman42 [59]

Answer:

i need help!!!!!!

Explanation:

3 0

4 years ago

اريد اجابتهم الذي بصوره وشكرا

11Alexandr11 [23.1K]

Answer:

ummm is the language urdu?????

5 0

2 years ago

To liquify a fixed amount of gas, one may 1. increase the temperature while decreasing the pressure. 2. increase the volume whil

antoniya [11.8K]

The complete question is:

To liquify a fixed amount of gas, one may 1. increase the temperature while decreasing the pressure. 2. increase the volume while increasing the pressure. 3. decrease the temperature while decreasing the pressure. 4. decrease the temperature while increasing the pressure. 5. decrease the volume while decreasing the pressure.

Answer:

4. decrease the temperature while increasing the pressure

Explanation:

The thermodynamics explains the sate of a substance (generally a gas or a liquid), which is its characteristics: temperature, pressure, volume, enthalpy, etc. When they changed, the state changes. Some of these changes may induce a physical change.

A gas has distant and agitated molecules, thus, the pressure is low and the temperature is higher, and a liquid has more close and less agitated molecules, so with higher pressure and low temperature.

Thus, to liquefy a fixed amount of has one may decrease the temperature while increasing the pressure.

6 0

3 years ago

An unknown compound was found to have a percent composition as follows: 47.0%, 14.5 carbon, and 38.5 oxygen. What is its empiric

shusha [124]

KCO₂

K₂C₂O₄

Explanation:

Given parameters:

Percent composition:

K = 47%

C = 14.5%

O = 38.5%

Molar mass of compound = 166.22g/mol

Unknown:

Empirical formula of compound = ?

Molecular formula of compound = ?

Solution:

The empirical formula of a compound is its simplest formula. Here is how to solve for it:

K C O

Percent

composition 47 14.5 38.5

Molar mass 39 12 16

Number

of moles 47/39 14.5/12 38.5/16

moles 1.205 1.208 2.4

Dividing

by smallest 1.205/1.205 1.208/1.205 2.4/1.205

1 1 2

Empirical formula KCO₂

Molecular formula

This is the actual combination of the atoms:

Molecular formula = ( empirical formula of KCO₂)ₙ

Molar mass of empirical formula = 39 + 12 + 2(16) = 83g/mol

n factor = $\frac{true molecular mass}{molar mas of empirical formula}$

n factor = $\frac{166.22}{83}$ = 2

Molecular formula of compound = ( KCO₂)₂ = K₂C₂O₄

Learn more:

Empirical formula brainly.com/question/2790794

#learnwithBrainly

6 0

4 years ago